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CBSE 12th Standard Chemistry Subject Solution Case Study Questions With Solution 2021

By QB365 on 21 May, 2021

QB365 Provides the updated CASE Study Questions for Class 12 , and also provide the detail solution for each and every case study questions . Case study questions are latest updated question pattern from NCERT, QB365 will helps to get  more marks in Exams

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12th Standard CBSE

Final Semester - June 2015

Read the passage given below and answer the following questions: The concentration of a solute is very important in studying chemical reactions because it determines how often molecules collide in solution and thus indirectly determine the rate of reactions and the conditions at equilibrium. There are several ways to express the amount of solute present in a solution. The concentration of a solution is a measure of the amount of solute that has been dissolved in a given amount of solvent or solution. Concentration can be expressed in terms of molarity, molality, parts per million, mass percentage, volume percentage, etc. The following questions are multiple choice questions. Choose the most appropriate answer: (i) The molarity (in mol L -1 ) of the given solution will be

(ii) Which of the following is correct relationship between mole fraction and molality?

(iii) Which of the following is temperature dependent?

(iv) Which of the following is true for an aqueous solution of the solute in terms of concentration?

Read the passage given below and answer the following questions: At 298 K, the vapour pressure of pure benzene, C 6 H 6 is 0.256 bar and the vapour pressure of pure toluene C 6 H 5 CH 3 is 0.0925 bar. Two mixtures were prepared as follows: (i) 7.8 g of C 6 H 6 + 9.2 g of toluene (ii) 3.9 g of C 6 H 6 + 13.8 g of toluene The following questions are multiple choice questions. Choose the most appropriate answer: (i) The total vapour pressure (bar) of solution 1 is

(ii) Which of the given solutions have higher vapour pressure?

(iii) Mole fraction of benzene in vapour phase in solution 1 is

(iv) Solution I is an example of a/an

Read the passage given below and answer the following questions: An ideal solution may be defined as the solution which obeys Raoult's law exactly over the entire range of concentration. The solutions for which vapour pressure is either higher or lower than that predicted by Raoult's law are called non-ideal solutions. Non-ideal solutions can show either positive or negative deviations from Raoult's law depending on whether the A-B interactions in solution are stronger or weaker than A - A and B - B interactions. The following questions are multiple choice questions. Choose the most appropriate answer: (i) Which of the following solutions is/are ideal solution(s)? (i) Bromoethane and iodoethane (ii) Acetone and chloroform (iii) Benzene and acetone (iv)n-heptane and n-hexane

(ii) Which of the following is not true for positive deviations?

(iii) For water and nitric acid mixture which of the given graph is correct?

(iv) Water- HCl mixture I. shows positive deviations  II. forms minimum boiling azeotrope III. shows negative deviations  IV. forms maximum boiling azeotrope

Read the passage given below and answer the following questions: The properties of the solutions which depend only on the number of solute particles but not on the nature of the solute are called colligative properties. Relative lowering in vapour pressure is also an example of colligative properties. For an experiment, sugar solution is prepared for which lowering in vapour pressure was found to be 0.061 mm of Hg. (Vapour pressure of water at 20°C is 17.5 mm of Hg.) The following questions are multiple choice questions. Choose the most appropriate answer: (i) Relative lowering of vapour pressure for the given solution is

(ii) The vapour pressure (mm of Hg) of solution will be

(iii) Mole fraction of sugar in the solution is

(iv) The vapour pressure (mm of Hg) of water at 293 K when 25 g of glucose is dissolved in 450 g of water is

Read the passage given below and answer the following questions: Few colligative properties are: (a) relative lowering of vapour pressure: depends only on molar concentration of solute (mole fraction) and independent of its nature. (b) depression in freezing point: it is proportional to the molal concentration of solution. (c) elevation of boiling point: it is proportional to the molal concentration of solute. (d) osmotic pressure: it is proportional to the molar concentration of solute. A solution of glucose is prepared with 0.052 g at glucose in 80.2 g of water. (K f = 1.86 K kg mol -1  and K b = 5.2 K kg mol -1 ) The following questions are multiple choice questions. Choose the most appropriate answer: (i) Molality of the given solution is

(ii) Boiling point for the solution will be

(iii) The depression in freezing point of solution will be

(iv) Mole fraction of glucose in the given solution is

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Cbse 12th standard chemistry subject solution case study questions with solution 2021 answer keys.

(i) (d) : Density of solution = 1.202 g/mL Volume of solution =  \(\frac{100 \mathrm{~g}}{1.202 \mathrm{~g} / \mathrm{mL}}=83.2 \mathrm{~mL}\) Molarity =  \(\frac{n_{\mathrm{KI}}}{\text { Volume of solution in } \mathrm{L}}\) \(=\frac{0.120 \mathrm{~mol}}{0.0832 \mathrm{~L}}=1.4423 \mathrm{~mol} \mathrm{~L}^{-1}\) (ii) (a):  \(x_{2}=\frac{n_{2}}{n_{1}+n_{2}} ; x_{1}=\frac{n_{1}}{n_{1}+n_{2}} ; \frac{x_{2}}{x_{1}}=\frac{n_{2}}{n_{1}}\) \(\frac{x_{2}}{x_{1}}=\frac{m_{2} / M_{2}}{m_{1} / M_{1}}=\frac{m_{2}}{m_{1}} \times \frac{M_{1}}{M_{2}}\)           ...(i) Molality =  \(\frac{n_{2}}{m_{1}}=\frac{m_{2}}{M_{2} \times m_{1}}\)               ...(ii) From(i) and (ii), m =  \(\frac{x_{2}}{x_{1}} \times \frac{1}{M_{1}} ; x_{1}=1-x_{2}\) Hence. x 2  =  \(\frac{m M_{1}}{1+m M_{1}}\) (iii) (a) : Mass does not depend on temperature while volume does. Hence, molarity depends on temperature. (iv) (b): 1M solution contains 1 mole of solute in less than 1000 g of the solvent whereas 1 m solution has 1 mole of the solute in 1000 g of the solvent.

(i) (b) : Moles of C 6 H 6  =  \(\frac{7.8}{78}=0.1\) Mole C 6 H 5 CH 3  =  \(\frac{9.2}{92}=0.1\) Mole fraction of C 6 H 6  =  \(\frac{0.1}{0.1+0.1}=0.5\) => Mole fraction of C 6 H 5 CH 3 = 0.5 Vapour pressure of toluene = Vapour pressure of pure toluene x mole fraction of toluene = 0.0925 x 0.5 = 0.04625 Vapour pressure of benzene = 0.256 x 0.5 = 0.128 Total vapour pressure of solution = 0.17425 (ii) (a) :  Moles of benzene in solution-II =  \(\frac{3.9}{78}=0.05\) Moles of toluene in solution-II =  \(\frac{13.8}{92}=0.15\) Vapour pressure of solution = 0.256 x 0.05 + 0.0925 x 0.15 = 0.0128 + 0.013875 = 0.026675 (iii) (c) : Mole fraction of benzene in vapour phase \(y_{\text {benzene }}=\frac{p_{\text {benzene }}}{P_{\text {total }}}=\frac{0.128}{0.17425}=0.734\) (iv) (a) : Benzene and toluene form an ideal solution.

(i) (d) : II represents negative deviations and III represents positive deviations. (ii) (b): For positive deviations  \(p_{A}>p_{A}^{\circ} x_{A} \text { and } p_{B}>p_{B}^{\circ} x_{B}\) (iii) (b) : Water and nitric acid mixture shows negative deviations from Raoult's law, hence  \(p_{A}<p_{A}^{\circ} x_{A} \text { and } p_{B}<p_{B}^{\circ} x_{B}\) (iv) (d): Water-HCl mixture shows negative deviations from Raoult's law and solutions showing negative deviations from ideal behaviour form maximum boiling azeotrope.

(i) (a) : Vapour pressure of water  \(\left(p_{A}^{\circ}\right)\)  = 17.5 mm of Hg Lowering of vapour pressure  \(\left(p_{A}^{\circ}-p_{A}\right)\) = 0.061 Relative lowering of vapour pressure   \(=\frac{p_{A}^{\circ}-p_{A}}{p_{A}^{\circ}}=\frac{0.061}{17.5}=0.00348\) (ii) (c): P = Vapour pressure of solvent - lowering in vapour pressure = 17.5 - 0.061 = 17.439 mm of Hg (iii) (a):  \(\frac{p_{A}^{\circ}-p_{A}}{p_{A}^{\circ}}=x_{B}=0.00348\) Hence, mole fraction of sugar = 0.00348 (iv) (b):  \(\frac{p_{A}^{\circ}-p_{A}}{p_{A}^{\circ}}=x_{B}=\frac{w_{B} \times M_{A}}{M_{B} \times w_{A}}\) \(\frac{17.5-p_{A}}{17.5}=\frac{25 \times 18}{450 \times 180}=5.56 \times 10^{-3}\) \(17.5-p_{A}=17.5 \times 5.56 \times 10^{-3}\) \(17.5-p_{A}=0.0973\) P = 17.40 mm Hg

(i) (b) : m  \(=\frac{0.052}{180} \times \frac{1000}{80.2}=0.0036\) (ii) (c):   \(\Delta T_{b}=K_{b} \times m=5.2 \times 0.0036=0.0187 \mathrm{~K}\) \(T_{b}=373+0.0187=373.0187 \mathrm{~K} \approx 373.02 \mathrm{~K}\) (iii) (d):  \(\Delta T_{f}=K_{f} \times m=1.86 \times 0.0036=0.067 \mathrm{~K}\) (iv) (a): Moles of glucose  \(=\frac{0.052}{180}=0.00028\) Moles 0f water =  \(\frac{80.2}{18}=4.455\) Mole fraction of glucose =  \(\frac{0.00028}{4.45+0.00028}=6.28 \times 10^{-5}\)

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Case Study Questions for Class 12 Chemistry Chapter 2 Solutions

• Last modified on: 4 weeks ago
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Table of Contents

There is Case Study Questions in class 12 Chemistry in session 2020-21. For the first time, the board has introduced the case study questions in the board exam. The first two questions in the board exam question paper will be based on Case Study and Assertion & Reason. The first question will have 5 MCQs out of which students will have to attempt any 4 questions. The second question will carry 5 Assertion & Reason type questions with the choice to attempt any four. Here are the questions based on case study.

Case Study Question 1:

Read the passage given below and answer the following questions:

The properties of the solutions which depend only on the number of solute particles but not on the nature of the solute are called colligative properties. Relative lowering in vapour pressure is also an example ofcolligative properties.

For an experiment, sugar solution is prepared for which lowering in vapour pressure was found to be 0.061 mm of Hg. (Vapour pressure of water at 20 0 C is 17.5 mm of Hg)

The following questions are multiple choice questions. Choose the most appropriate answer:

(i) Relative lowering of vapour pressure for the given solution is (a) 0.00348 (b) 0.061 (c) 0.122 (d) 1.75

(ii) The vapour pressure (mm of Hg) of solution will be (a) 17.5 (b) 0.61 (c) 17.439 (d) 0.00348

(iii) Mole fraction of sugar in the solution is (a) 0.00348 (b) 0.9965 (c) 0.061 (d) 1.75

If weight of sugar taken is 5 g in 108 g of water then molar mass of sugar will be (a) 358 (b) 120 (c) 240 (d) 400

(iv) The vapour pressure (mm of Hg) of water at 293K when 25g of glucose is dissolved in 450 g of water is (a) 17.2 (b) 17.4 (c) 17.120 (d) 17.02

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Case Study on Solutions Class 12 Chemistry PDF

Better preparation of Case Study on Solutions Class 12 Chemistry can help students score good marks in the CBSE Class 12 Board examination. Additionally, it helps build confidence and enables students to deepen their knowledge of Solutions. Because case-based questions are equally important for learning and board exam preparation, our team has prepared Case Study on Solutions Class 12 Chemistry in a PDF file for free distribution among students.

Links to download the PDF file of the Solutions Case Study for Class 12 Chemistry free of cost are mentioned on this page.

Solutions Case Study for Class 12 Chemistry with Solutions in PDF

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4 Tips to Answer Class 12 Chemistry Solutions Case Study Questions?

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• Read the Case Carefully: To start gathering insights from the given case-based questions, it is vital to read the Solutions case carefully and identify the key facts, figures, and units of measurement. Pay attention to any diagrams or graphs related to Solutions provided, as they may contain important information.
• Identify the Problem: While reading the Solutions case it is essential to consider the possible causes and effects. This will help you determine the appropriate approach to solving the problem in Class 12 Chemistry Solutions.
• Use Elimination Methods Too: Since case study questions of Class 12 Chemistry Solutions, are often framed in Multiple choice questions, students should have the knowledge of elimination methods in MCQs to better answer the questions.
• Before All, Master the Concept of Solutions: If the above two methods are not working for you to answer Case Study on Solutions Class 12 Chemistry then you need to revisit the lesson and master the concepts explained in the Solutions Class 12 Chemistry.

What is the Benefit of Practising Class 12 Chemistry Solutions Case Study Questions?

When a student decides to practise Class 12 Chemistry Solutions case study questions before the board examination they generally get these 3 benefits:

• Quick Conceptual Revision: Nothing is better for revision than solving relevant questions and therefore, those who involve in solving the Solutions Case study questions before the Class 12 Chemistry exam are able to better revise their conceptual learnings from the lesson.
• Better Board Exam Preparation: No doubt, the more you practise Solutions case study questions the better your exam preparation will be so, solving Case-based questions prior to the board examination helps a lot in the preparation. It also enables the students to know what are the Solutions questions which have the possibility to be asked in the board examination.
• Confident in Using Analytical or Critical Thinking Skills: The Case-based questions on Solutions are all about using analytical or critical thinking skills where students are required to solve problems based on the situations or data given. Thus, practising Case Study on Solutions Class 12 Chemistry benefits students to feel confident and comfortable in using analytical skills.

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Case Study Questions Class 12 Chemistry

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Download the app to get CBSE Sample Papers 2023-24, NCERT Solutions (Revised), Most Important Questions, Previous Year Question Bank, Mock Tests, and Detailed Notes.

CBSE will ask Case Study Questions class 12 Chemistry in session 2020-21. These will be the first two questions in the board exam question paper. The first question will have 5 MCQs out of which students will attempt any 4 questions. The second question will carry 5 Assertion & Reason type questions with the choice to attempt any four.

Case Study Questions

As you know, CBSE will hold exams in May-June this year. There is already a reduction of 30% in the syllabus. Now, the case study questions have been added. So, this year the question paper is going to be a bit easier. Although it is easy yet these case study questions need special attention and regular practice.

We have added around 10 sample questions based on the latest pattern in myCBSEguide App. These all questions include two case study questions.

Class 12 Chemistry Question Bank

If you go through the previous year question papers, you will analyze that many questions are repeated word by word and many others are almost similar. So, it is always recommended to check all questions asked in previous years. This will not only help you to get an idea about the question pattern but also help you to understand the difficulty level of the questions.

myCBSEguide App has the previous year’s question bank. These questions are arranged chapter-wise. If you are preparing a particular chapter, you will get all questions asked from that chapter in the last 10 years.

Case Study Questions Examples

Here are two examples of case study questions. To get more such questions download the myCBSEguide App and browse Sample Papers there.

Read the passage given below and answer any four out of the following questions: Ammonia is present in small quantities in air and soil where it is formed by the decay of nitrogenous organic matter e.g., urea. On a large scale, ammonia is manufactured by Haber’s process. In accordance with Le Chatelier’s principle, high pressure would favour the formation of ammonia. Ammonia is a colourless gas with a pungent odour. Its freezing and boiling points are 198.4 and 239.7 K respectively. In the solid and liquid states, it is associated through hydrogen bonds as in the case of water and that accounts for its higher melting and boiling points than expected on the basis of its molecular mass. Ammonia gas is highly soluble in water. Its aqueous solution is weakly basic due to the formation of OH– ions. The presence of a lone pair of electrons on the nitrogen atom of the ammonia molecule makes it a Lewis base.

• caustic soda
• calcium chloride
• sodium hydroxide
• sodium chloride
• ​200 10 5 Pa
• 400 10 5 Pa
• 100 10 5 Pa
• 300 10 5 Pa
• Mg 2 O 3  + K 2 O
• Al 2 O 3  + K 2 O
• NaO 3  + K 2 O
• None of these
• five bond pair and two lone pair
• four lone pair and one bond pair
• three bond pair and one lone pair
• three bond pair and two lone pair

Read the passage and answer any four out of the following questions: Colloidal particles always carry an electric charge. The nature of this charge is the same on all the particles in a given colloidal solution and may be either positive or negative. The charge on the sol particles is due to one or more reasons, viz., due to electron capture by sol particles during electrodispersion of metals. When two or more ions are present in the dispersion medium, preferential adsorption of the ion common to the colloidal particle usually takes place. When silver nitrate solution is added to the potassium iodide solution, the precipitated silver iodide adsorbs iodide ions from the dispersion medium, and negatively charged colloidal solution results. acquired a positive or a negative charge by selective adsorption on the surface of a colloidal particle The combination of the two layers of opposite charges around the colloidal particle is called Helmholtz electrical double layer. The presence of equal and similar charges on colloidal particles is largely responsible for providing stability to the colloidal solution.

In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices. 

• Assertion and reason both are correct statements and reason is correct explanation for assertion
• Assertion and reason both are correct statements but reason is not correct explanation for assertion
• Assertion is correct statement and reason is wrong statement
• Assertion is wrong statement but reason is correct statement
• Assertion:  The presence of equal and similar charges on colloidal particles is largely responsible in providing stability to the colloidal solution. Reason:  The repulsive forces between charged particles having the same charge prevent them from aggregating and provide stability.
• Assertion: The first layer is mobile in Helmholtz electrical double layer. Reason:  The potential difference between the fixed layer and the diffused layer of opposite charges is called zeta potential.
• Assertion: The sol particle in colloid has a charge. Reason:  The charge in sol is due to electron capture by sol particles during the electrodispersion of metals.
• Assertion:  Methylene blue sol is a negatively charged sol. Reason: When KI solution is added to AgNO 3 solution, positively charged sol formed.
• Assertion:  If FeCl3 is added to an excess of hot water, a positively charged sol of hydrated ferric oxide is formed. Reason: When ferric chloride is added to NaOH a negatively charged sol is obtained with adsorption of OH- ions.

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CBSE Class 12 Chemistry Case study Questions & Answers For Chapter 1, 2, 4, 6, 7, 8, 9, 10, 11, 12, 13, 14, 15, 16

Understudies can discover the chapter astute vital questions for course 12th Chemistry within the table underneath. These imperative questions incorporate questions that are regularly inquired in a long time. Moreover, arrangements are to give for these questions, with extraordinary accentuation on ease-of-study. Tap on the joins underneath to begin investigating.

Below we posted all the Case Study Questions & Answers for Class 12 Chemistry all Chapters –

CBSE Class 12 Case Study Question for Chemistry

Case study 1.

(1) Read the passage given below and answer the questions that follow.

 Are there nuclear reactions going on in our bodies?

There are nuclear reactions constantly occurring in our bodies, but there are very few of them compared to the chemical reactions, and they do not affect our bodies much. All of the physical processes that take place to keep a human body running are chemical processes. Nuclear reactions can lead to chemical damage, which the body may notice and try to fix. The nuclear reaction occurring in our bodies is radioactive decay. This is the change of a less stable nucleus to a more stable nucleus. Every atom has either a stable nucleus or an unstable nucleus, depending on how big it is and on the ratio of protons to neutrons. The ratio of neutrons to protons in a stable nucleus is thus around 1:1 for small nuclei (Z < 20). Nuclei with too many neutrons, too few neutrons, or that are simply too big are unstable. They eventually transform to a stable form through radioactive decay. Wherever there are atoms with unstable nuclei (radioactive atoms), there are nuclear reactions occurring naturally. The interesting thing is that there are small amounts of radioactive atoms everywhere: in your chair, in the ground, in the food you eat, and yes, in your body.

The most common natural radioactive isotopes in humans are carbon-14 and potassium-40. Chemically, these isotopes behave exactly like stable carbon and potassium. For this reason, the body uses carbon-14 and potassium-40 just like it does normal carbon and potassium; building them into the different parts of the cells, without knowing that they are radioactive. In time, carbon-14 atoms decay to stable nitrogen atoms and potassium-40 atoms decay to stable calcium atoms. Chemicals in the body that relied on having a carbon-14 atom or potassium-40 atom in a certain spot will suddenly have a nitrogen or calcium atom. Such a change damages the chemical. Normally, such changes are so rare, that the body can repair the damage or filter away the damaged chemicals. The natural occurrence of carbon-14 decay in the body is the core principle behind carbon dating. As long as a person is alive and still eating, every carbon-14 atom that decays into a nitrogen atom is replaced on average with a new carbon-14 atom. But once a person dies, he stops replacing the decaying carbon-14 atoms. Slowly the carbon-14 atoms decay to nitrogen without being replaced, so that there is less and less carbon-14 in a dead body. The rate at which carbon-14 decays is constant and follows first order kinetics. It has a half – life of nearly 6000 years, so by measuring the relative amount of carbon-14 in a bone, archeologists can calculate when the person died. All living organisms consume carbon, so carbon dating can be used to date any living organism, and any object made from a living organism. Bones, wood, leather, and even paper can be accurately dated, as long as they first existed within the last 60,000 years. This is all because of the fact that nuclear reactions naturally occur in living organisms. (source: The textbook Chemistry: The Practical Science by Paul B. Kelter, Michael D. Mosher and Andrew Scott states)

(a)  Why is Carbon -14 radioactive while Carbon -12 not? (Atomic number of Carbon: 6)

Ans: Ratio of neutrons to protons is 2.3: 1 which is not the stable ratio of 1:1

(b) Researchers have uncovered the youngest known dinosaur bone, dating around 65 million years ago. How was the age of this fossil estimated?

Ans: Age of fossils can be estimated by C-14 decay. All living organisms have C-14 which decays without being replaced back once the organism dies.

(c)  Which are the two most common radioactive decays happening in human body?

Ans: carbon-14 atoms decay to stable nitrogen atoms and potassium-40 atoms decay to stable calcium.

(d) Suppose an organism has 20 g of Carbon -14 at its time of death. Approximately how much Carbon -14 remains after 10,320 years? (Given antilog 0.517 = 3.289)

Ans: t = 2.303/ k log (Co/Ct)

Co = 20 g Ct = ?

t = 10320 years k = 0.693/6000 (half-life given in passage)

substituting in equation:

10320 = 2.303 / (0.693/6000) log 20/ Ct

0.517 = log 20 / Ct anlilog (0.517) = 20/Ct

3.289 = 20/Ct

Ct = 6.17 g

(d) Approximately how old is a fossil with 12 g of Carbon -14 if it initially possessed 32 g of Carbon -14? (Given log 2.667 = 0.4260)

Co = 32 g Ct = 12

t = ? k = 0.693/6000 (half life given in passage) substituting in equation:

t = 2.303 / (0.693/6000) log 32/ 12

t = 2.303 x 60000 /0.693 log 2.667

t = 2.303x6000x0.4260 /0.693

= 8494 years

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Class 12 Chemistry Case Study Questions PDF Download

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Looking for Class 12 Chemistry Case Study Based Questions in PDF format? This comprehensive article provides expert insights, engaging content, and answers to frequently asked questions to help you excel in your studies. Download the PDF now and boost your chemistry knowledge!

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You need to improve your preparation for the Class 12 Chemistry Case Study Questions exams if you want to achieve a 95+% on the boards. You may find case study questions from every chapter that will be covered in the CBSE Class 12 Chemistry Board Exams in this post.

Table of Contents

Case Study-Based Questions for Class 12 Chemistry

Welcome to the world of Class 12 Chemistry Case Study Questions! As a student pursuing Chemistry in the 12th grade, you have already shown dedication and commitment to the subject. However, dealing with case study-based questions can be both intriguing and challenging. In this article, we will explore the nuances of such questions and offer valuable guidance to excel in your exams.

Class 12 Physics Case Study Questions Class 12 Chemistry Case Study Questions Class 12 Biology Case Study Questions Class 12 Maths Case Study Questions

Importance of Class 12 Chemistry Case Study-Based Questions

Class 12 Chemistry case study-based questions play a vital role in your overall understanding of the subject. They enable you to:

• Apply Theoretical Knowledge : Case studies allow you to apply the concepts you have learned in real-life situations, bridging the gap between theory and practical application.
• Develop Analytical Skills : By critically analyzing case scenarios, you enhance your analytical abilities, which are essential in various professional fields.
• Enhance Problem-Solving Abilities : Tackling case study-based questions hones your problem-solving skills, preparing you to face challenges with confidence.
• Gain Deeper Insights : Exploring different case studies exposes you to a wide range of chemical reactions and phenomena, broadening your understanding of Chemistry.

Tips to Excel in Class 12 Chemistry Case Study Questions

• Thoroughly Understand the Concepts: Before attempting case study questions, ensure you have a strong grasp of the underlying concepts and theories.
• Analyze the Scenario Carefully: Take your time to read and comprehend the given case study. Pay attention to every detail to identify the key points.
• Relate to Real-Life Scenarios: Try to connect the case study with real-life situations, as this will make the problem-solving process more intuitive.
• Practice Regularly: Practice a wide variety of case study questions to familiarize yourself with different scenarios and improve your problem-solving skills.
• Collaborate with Peers: Engage in group discussions and brainstorming sessions with your peers. This will provide diverse perspectives and enhance your critical thinking.

Best Books for Class 12 Chemistry

Strictly in accordance with the new term-by-term curriculum for the Class 12 Chemistry Case Study Questions exams to be held in the academic session 2024, including the new board-introduced multiple-choice question types, Stand-Alone MCQs, and MCQs based on Assertion-Reason Case-based MCQs. Included are inquiries from the official CBSE Question Bank that was released in April 2024. What changes have been made to the book: strictly in accordance with the term-by-term syllabus for the board exams that will be held during the 2024 academic year? Chapter- and topic-specific multiple-choice questions based on the unique assessment plan for the Class 12 Chemistry Case Study Questions Board Examination.

Chemistry Syllabus for 2024

Unit II: Solutions (15 Periods)

Types of solutions, expression of concentration of solutions of solids in liquids, solubility of gases in liquids, solid solutions, Raoult’s law, colligative properties – relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure, determination of molecular masses using colligative properties, abnormal molecular mass, Van’t Hoff factor.

Unit III: Electrochemistry (18 Periods)

Redox reactions, EMF of a cell, standard electrode potential, Nernst equation and its application to chemical cells, Relation between Gibbs energy change and EMF of a cell, conductance in electrolytic solutions, specific and molar conductivity, variations of conductivity with concentration, Kohlrausch’s Law, electrolysis and law of electrolysis (elementary idea), dry cell-electrolytic cells and Galvanic cells, lead accumulator, fuel cells, corrosion.

Unit IV: Chemical Kinetics (15 Periods)

Rate of a reaction (Average and instantaneous), factors affecting rate of reaction: concentration, temperature, catalyst; order and molecularity of a reaction, rate law and specific rate constant, integrated rate equations and half-life (only for zero and first order reactions), concept of collision theory (elementary idea, no mathematical treatment), activation energy, Arrhenius equation.

Unit VIII: d and f Block Elements (18 Periods)

General introduction, electronic configuration, occurrence and characteristics of transition metals, general trends in properties of the first-row transition metals – metallic character, ionization enthalpy, oxidation states, ionic radii, colour, catalytic property, magnetic properties, interstitial compounds, alloy formation, preparation and properties of K 2 Cr 2 O 7  and KMnO 4 .

Lanthanoids –  Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction and its consequences.

Actinoids –  Electronic configuration, oxidation states and comparison with lanthanoids.

Unit IX: Coordination Compounds (18 Periods)

Coordination compounds – Introduction, ligands, coordination number, colour, magnetic properties and shapes, IUPAC nomenclature of mononuclear coordination compounds. Bonding, Werner’s theory, VBT, and CFT; structure and stereoisomerism, the importance of coordination compounds (in qualitative analysis, extraction of metals and biological system).

Unit X: Haloalkanes and Haloarenes (15 Periods)

Haloalkanes:  Nomenclature, nature of C–X bond, physical and chemical properties, optical rotation mechanism of substitution reactions.

Haloarenes:  Nature of C–X bond, substitution reactions (Directive influence of halogen in monosubstituted compounds only). Uses and environmental effects of – dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons, DDT.

Unit XI: Alcohols, Phenols and Ethers (14 Periods)

Alcohols:  Nomenclature, methods of preparation, physical and chemical properties (of primary alcohols only), identification of primary, secondary and tertiary alcohols, mechanism of dehydration, uses with special reference to methanol and ethanol.

Phenols:  Nomenclature, methods of preparation, physical and chemical properties, acidic nature of phenol, electrophilic substitution reactions, uses of phenols.

Ethers:  Nomenclature, methods of preparation, physical and chemical properties, uses.

Unit XII: Aldehydes, Ketones and Carboxylic Acids (15 Periods)

Aldehydes and Ketones:  Nomenclature, nature of carbonyl group, methods of preparation, physical and chemical properties, mechanism of nucleophilic addition, reactivity of alpha hydrogen in aldehydes, uses.

Carboxylic Acids:  Nomenclature, acidic nature, methods of preparation, physical and chemical properties; uses.

Unit XIII: Amines (14 Periods)

Amines:  Nomenclature, classification, structure, methods of preparation, physical and chemical properties, uses, identification of primary, secondary and tertiary amines

Diazonium salts:  Preparation, chemical reactions and importance in synthetic organic chemistry.

Unit XIV: Biomolecules (18 Periods)

Carbohydrates –  Classification (aldoses and ketoses), monosaccharides (glucose and fructose), D-L configuration oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch, cellulose, glycogen); Importance of carbohydrates.

Proteins –  Elementary idea of – amino acids, peptide bond, polypeptides, proteins, structure of proteins – primary, secondary, tertiary structure and quaternary structures (qualitative idea only), denaturation of proteins; enzymes.

Hormones –  Elementary idea excluding structure.

Vitamins –  Classification and functions.

Nucleic Acids:  DNA and RNA.

FAQ on Class 12 Chemistry Case Study Questions

Q: can i rely solely on class 12 chemistry case study based questions exam preparation.

Yes, case study-based questions are an essential part of your preparation. However, it is advisable to supplement them with other study materials and revision of theoretical concepts for comprehensive preparation.

Q: How often should I practice Class 12 Chemistry Case Study Based Questions?

Frequent practice is crucial for mastering case study-based questions. Set aside dedicated practice sessions and gradually increase the difficulty level of the questions.

Q: Can I discuss case study questions with my teachers?

Absolutely! Engaging with your teachers regarding case study questions will provide valuable insights and clarifications.

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Case Study Questions Haloalkanes and Haloarenes Class 12 Chemistry

        Case Study Questions Haloalkanes and Haloarenes Class 12 Chemistry

1. Read the passage given below and answer the following questions: Nucleophilic substitution reactions are of two types; substitution nucleophilic bimolecular (S N 2) and substitution nucleophilic unimolecular (S N 1) depending on molecules taking part in determining the rate of reaction. The reactivity of alkyl halide towards S N 1 and S N 2 reactions depends on various factors such as steric hindrance, stability of intermediate or transition state, and polarity of the solvent. S N 2 reaction mechanism is favoured mostly by primary alkyl halide or transition state and polarity of the solvent, S N 2 reaction mechanism is favoured mostly by primary alkyl halide then secondary and then tertiary. This order is reversed in the case of S N 1 reactions. (i) Which of the following is most reactive towards nucleophilic substitution reaction? (a) C 6 H 5 Cl (b) CH 2 = CHCl (c) ClCH 2 CH = CH 2 (d) CH 3 CH = CHCl

(ii) Isopropyl chloride undergoes hydrolysis by (a) S N 1 mechanism (b) S N 2 mechanism (c) S N 1 and S N 2 mechanism (d) Neither S N 1 nor S N 2 mechanism

(iii) Tertiary alkyl halides are practically inert to substitution by S N 2 mechanism because of (a) Insolubility (b) Instability (c) Inductive effect (d) Steric Hindrance

(iv) Which of the following is the correct order of decreasing S N 2 reactivity? (a) RCH 2 X > R 2 CHX > R 3 CX (b) R 3 CX > R 2 CHX >RCH 2 X (c) R 2 CHX > R 3 CX > RCH 2 X (d) RCH 2 X > R 3 CX > R 2 CHX

(v) An organic molecule necessarily shows optical activity if it- a) Contains asymmetric carbon atoms b) Is non-polar c) Is non-superimposable on its mirror image d) Is superimposable on its mirror image.

2. Read the passage given below and answer the following questions: The replacement of hydrogen atom in a hydrocarbon, aliphatic or aromatic results in the formation of haloalkanes and haloarenes respectively. Haloalkanes contain a halogen atom attached to sp 3 hybridized carbon atom of an alkyl group whereas haloarenes contain a halogen atom attached to sp 2 hybridized carbon atom of an aryl group. Haloalkanes and haloarenes may be classified on the basis of the number of halogen atoms in their structures as mono, di, or poly halogen compounds and also on the basis of the state of hybridization of the carbon atom to which the halogen atom is bonded. (i) Which of the following halide is 2°? (a) Isopropyl chloride (b) Isobutyl chloride (c) n-propyl chloride (d) n-butyl chloride

(ii) Which of the following is a Gem-dibromide is: (a) CH 3 CH(Br)CH 2 (Br) (b) CH 3 CBr 2 CH 3 (c) CH 2 (Br)CH 2 CH 2 (d) CH 2 BrCH 2 Br

(iii) IUPAC name of (CH 3 ) 3 CCl is: (a) 3-Chlorobutane (b) 2-Chloro-2-methylpropane (c) t-butyl chloride (d) n-butyl chloride

(iv) Which of the following is a primary halide? (a) Isopropyl iodide (b) Secondary butyl iodide (c) Tertiarybutyl bromide (d) Neohexyl chloride

(v) Which one of the following is not an allylic halide? (a) 4-Bromopent-2-ene (b) 3-Bromo-2-methylbut-1-ene (c) 1-Bromobut-2-ene (d) 4-Bromobut-1-ene

3. Read the passage given below and answer the following questions: Alkyl halides are prepared by the free radical halogenation of alkanes, addition of halogen acids to alkenes, replacement of -OH group of alcohols with halogens using phosphorus halides, thionyl chloride, or halogen acids. Aryl halides are prepared by electrophilic substitution to arene. Fluorine and iodides are best prepared by the halogen exchange method. These compounds find wide applications in industry as well as in day-to-day life. These compounds are generally used as solvents and as starting materials for the synthesis of a large number of organic compounds. (i) The best method for the conversion of an alcohol into an alkyl chloride is by treating the alcohol with (a) PCl 5 (b) Dry HCl in the presence of anhydrous ZnCl 2 (c) SOCl 2 in presence of pyridine (d) None of these

(ii) The catalyst used in the preparation of an alkyl chloride by the action of dry HCl on alcohol is (a) anhydrous AlCl 3 (b) FeCl 3 (c) anhydrous ZnCl 2 (d) Cu

(iii) An alkyl halide reacts with metallic sodium in dry ether. The reaction is known as: (a) Frankland’s reaction (b) Sandmeyer’s reaction (c) Wurtz reaction (d) Kolbe’s reaction

(iv) Fluorobenzene (C 6 H 5 F) can be synthesized in the laboratory (a) By direct fluorination of benzene with F 2 gas (b) By reacting bromobenzene with NaF solution (c) By heating phenol with HF and KF (d) From aniline by diazotization followed by heating the diazonium salt with HBF 4

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Question 1 - Case Based Questions - Chapter 1 Class 9 Economics - The Story of Village Palampur - Economics

Last updated at April 16, 2024 by Teachoo

Read the text given below and answer the following questions: 

 Palampur is well-connected with neighbouring  villages and towns. Raiganj, a big village, is 3 kms  from Palampur. An all-weather road connects the village to Raiganj and further on to the nearest  small town of Shahpur. This village has about 450  families belonging to several different castes. The  80 upper caste families own the majority of land in  the village. Their houses, some of them quite large,  are made of brick with cement plastering. The SCs  (dalits) comprise one third of the population and  live in one corner of the village and in much smaller  houses some of which are of mud and straw. Most  of the houses have electric connections. Electricity  powers all the tube wells in the fields and is used  in various types of small business. Palampur has  two primary schools and one high school. There is  a primary health centre run by the government and  one private dispensary where the sick is treated. The  story of Palampur, an imaginary village, will take us  through the different types of production activities  in the village. In villages across India, farming is  the main production activity. The other production  activities, referred to as non- farm activities include  small manufacturing, transport, shop-keeping, etc.  Every production is organised by combining land,  labour, physical capital and human capital, which  are known as factors of production. 

Question (i)

Raiganj, a big village, is  __________  kms from  palampur.  .

(a) 5 

(b) 4  

(c) 3 

(d) 1 

From the paragraph, 

Palampur is well-connected with neighbouring  villages and towns. Raiganj, a big village, is 3 kms  from Palampur. An all-weather road connects the village to Raiganj and further on to the nearest  small town of Shahpur. This village has about 450  families belonging to several different castes.

 (c) Raiganj, a big village, is  3  kms from  Palampur. 

Question (ii)

Which of the following statement is true with  respect to palampur:  .

(a) Palampur has one primary school and  two high schools.  

(b) Palampur has two primary schools and  one high school.  

(c) Dairy is the main production activity.  

(d) The village has about 600 families  belonging to several different castes. 

From the paragraph,

Electricity  powers all the tube wells in the fields and is used  in various types of small business . Palampur has  two primary schools and one high school . There is  a primary health centre run by the government and  one private dispensary where the sick is treated. The  story of Palampur, an imaginary village, will take us  through the different types of production activities  in the village.

Answer:  

(b) Palampur has two primary schools and  one high school. 

Question (iii)

Raw materials and money in hand are called:  .

(a) Working capital  

(b) Fixed capital  

(c) Human capital  

(d) None of the above  

Question (iv)

The variety of inputs required at every stage  during production is known as_________.  .

(a) Physical capital  

(b) Labour  

(d) None of the above 

(a) Physical capital 

Question (v)

How many primary schools and high schools do palampur has.

Electricity powers all the tube wells in the fields and is used in various types of small businesses. Palampur has two primary schools and one high school . There is a primary health center run by the government and one private dispensary where the sick are treated. The story of Palampur, an imaginary village, will take us through the different types of production activities in the village.

(a) Palampur has  two primary schools and one high school. 

Question (vi)

What are the factors of production.

In villages across India, farming is the main production activity. The other production activities, referred to as non-farm activities include small manufacturing, transport, shop-keeping, etc.  Every production is organized by combining land, labor, physical capital, and human capital, which are known as factors of production. 

Every production is organized by combining land, labor, physical capital, and human capital, which  are known as factors of production. 

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Case Study Questions for Class 12 Accountancy with Answers

Students should practice Case Study Questions for Class 12 Accountancy with Answers before appearing in Class 12 Accountancy Board exams. We have provided below the class 12 Accountancy Case Study questions based on each chapter in your NCERT Book for Class 12 Accountancy. These chapter-wise questions have been prepared by teachers based on the latest examination pattern and syllabus issued by CBSE, NCERT KVS. The following Case Study questions and answers will be really useful to understand the type of questions that can be asked in exams

Class 12 Accountancy Case Study Questions and Answers

Practicing by going through the past year and Case Study questions for CBSE Class 12 Accountancy is very important to prepare for the Grade 12 Accountancy exams. We have provided below the best collection of questions which can come in your exams.

Chapter Wise Important Questions for Class 12 Accountancy with Answers

It is important for students to go through Important Case Study Questions for Class 12 Accountancy with Answers regularly while studying various chapters. This will help students to test their understanding of various topics and also make sure that they have understood all topics properly. Our teachers have done a detailed analysis of all chapters in your NCERT Book for Class 12 Accountancy. They have identified all the important questions which they expect can come in the examinations.

Students should read the chapters and notes provided by us properly. Then they should refer to the chapter-wise questions given by us. We have covered all important and difficult topics and have provided answers to all Case Study questions. We have provided step-by-step solutions so that you are able to understand the concepts explained behind the questions.

Frequently asked questions by Class 12 Accountancy Students

You can download the best collection of Class 12 Accountancy questions and answers from https://cbsencertsolutions.com/. Our faculty has provided the most important questions which can be asked in exams.

Yes, all chapter-wise questions and answers have been prepared based on the latest syllabus issued by CBSE for the current academic year.

Apart from Accountancy for Class 12, we have provided notes and important questions for all other subjects in Class 12. You can read the online or download PDF

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Case Study Questions Class 9 Economics Chapter 3 Poverty as a Challenge

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Case study Questions in Class 9 Social Science Chapter 3 are very important to solve for your exam. Class 9 Social Science Chapter 10 Case Study Questions have been prepared for the latest exam pattern. You can check your knowledge by solving  case study-based questions for Case Study Questions Class 9 Economics Chapter 3 Poverty as a Challenge

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Poverty as a Challenge Case Study Questions With Answers

Here, we have provided case-based/passage-based questions for Class 9 Social Science Chapter 3 Poverty as a Challenge

Case Study 1: The proportion of people below the poverty line is also not the same for all social groups and economic categories in India. Social groups, which are most vulnerable to poverty are Scheduled Caste and Scheduled Tribe households. Similarly, among the economic groups, the most vulnerable groups are the rural agricultural labour households and the urban casual labour households. Although the average for people below the poverty line for all groups in India is 22. 43 out of 100 people belonging o Scheduled Tribes are not able to meet their basic needs. Similarly, 34 per cent of casual workers in urban areas are below the poverty line. About 34 per cent of casual labour farms (in rural areas) and 29 per cent of Scheduled castes are also poor. The double disadvantage of being a landless casual wage labour household in the socially disadvantaged social groups of the scheduled caste or the scheduled tribe population highlights the seriousness of the problem. Some recent studies have shown that except for the scheduled tribe households, all the other three groups (i.e., scheduled castes, rural agricultural labourers and urban casual labour households have seen a decline in poverty in the 1990s.

Which of the following factors are needed to determine the poverty line? (a) A minimum level of food requirement and clothing (b) A minimum level of consumption of fuel and light (c) A minimum level of education and medical facilities (d) All of the above

Answer: (d) All of the above

What is the reason behind vulnerability to poverty for the rural agricultural labour and urban casual labour? (a) They do not have their own lands/property (b) They only get seasonal work (c) They are poorly paid (d) All of the above

There is also inequality among the family members as (a) In poor families all suffer but some suffer more than others (b) Women, elderly and female infants are denied equal access to resources (c) Both (a) and (b) (d) None of the above

Answer: (c) Both (a) and (b)

Which of the following reason(s) is/are cause for declining poverty ratio? (a) Focusing on human resource development (b) Land reform measures (c) Both (a) and (b) (d) None of these

Which state in India has reduced poverty by taking human resource development? (a) Uttar Pradesh (b) Haryana (c) Tamil Nadu (d) None of the above

Answer: (d) None of the above

Which state can reduce poverty by improving its PDS system? (a) Andhra Pradesh (b) Tamil Nadu (c) Both (a) and (b) (d) None of the above

Case Study 2: Poverty is a significant challenge faced by many countries, including India. It refers to the lack of basic necessities and resources required for a decent standard of living. In India, poverty is measured using a poverty line, which is the minimum level of income required to meet the essential needs of an individual. Poverty can be classified into two categories: rural poverty and urban poverty. Rural poverty is primarily caused by factors such as low agricultural productivity, lack of access to credit, unemployment, and landlessness. Urban poverty, on the other hand, is attributed to factors like unemployment, low wages, lack of skill development, and migration from rural areas. Poverty not only affects the material well-being of individuals and families but also leads to social exclusion and limited access to education, healthcare, and other essential services. Addressing poverty requires comprehensive measures such as poverty alleviation programs, inclusive economic growth, skill development, and social welfare initiatives.

How is poverty measured in India? a) By the level of education attained by individuals b) By the amount of land owned by individuals c) By the minimum level of income required to meet essential needs d) By the number of family members in a household

Answer: c) By the minimum level of income required to meet essential needs

What are the two categories of poverty in India? a) Agricultural poverty and industrial poverty b) Rural poverty and urban poverty c) Primary poverty and secondary poverty d) Absolute poverty and relative poverty

Answer: b) Rural poverty and urban poverty

What are some factors contributing to rural poverty in India? a) Lack of access to credit and low agricultural productivity b) High wages and lack of skill development c) Industrialization and urbanization d) Availability of agricultural subsidies

Answer: a) Lack of access to credit and low agricultural productivity

Which of the following factors is attributed to urban poverty in India? a) High wages and skill development b) Lack of access to credit and low agricultural productivity c) Industrialization and urbanization d) Availability of agricultural subsidies

Answer: c) Industrialization and urbanization

Besides material well-being, what are some consequences of poverty? a) Increased access to education and healthcare b) Social exclusion and limited access to essential services c) Higher standard of living and improved infrastructure d) Reduced income inequality and social mobility

Answer: b) Social exclusion and limited access to essential services

Hope the information shed above regarding Case Study and Passage Based Questions for Class 9 Social Science Chapter 3 Poverty as a Challenge with Answers Pdf free download has been useful to an extent. If you have any other queries about CBSE Class 9 Social Science Poverty as a Challenge Case Study and Passage-Based Questions with Answers, feel free to comment below so that we can revert back to us at the earliest possible By Team Study Rate

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Case Study Questions of Chapter 3 Atoms and Molecules PDF Download

Case study Questions on Class 9 Science Chapter 3  are very important to solve for your exam. Class 9 Science Chapter 3 Case Study Questions have been prepared for the latest exam pattern. You can check your knowledge by solving case study-based questions for Class 9 Science Chapter 3 Atoms and Molecules

In CBSE Class 9 Science Paper, Students will have to answer some questions based on Assertion and Reason. There will be a few questions based on case studies and passage-based as well. In that, a paragraph will be given, and then the MCQ questions based on it will be asked.

Atoms and Molecules Case Study Questions With answers

Here, we have provided case-based/passage-based questions for Class 9 Science  Chapter 3 Atoms and Molecules

Case Study/Passage Based Questions

The knowledge of valencies of various radicals helps us to write the formulae of chemical compounds. The total positive charge on positive ions (cations) is equal to the total negative charge on negative ions (anions) in a molecule. Therefore, in writing the formula of a compound, the positive and negative ions are adjusted in such a way that the total number of positive charges of positive ions (cations) becomes equal to the total number of negative charges of negative ions (anions). There is another simple method for writing the formulae of ionic compounds. In this method, the valencies (or positive or negative charges) of the ions can be ‘crossed over’ to give subscripts. The purpose of crossing over of charges is to find the number of ions required to equalise the number of positive and negative charges.

Element X has two valencies 5 and 3 and Y has valency 2. The elements X and Y are most likely to be respectively (a) copper and sulphur (b) sulphur and iron (c) phosphorus and fluorine (d) nitrogen and iron.

Answer: (d) nitrogen and iron.

The formula of the sulphate of an element X is X 2 (SO 4 ) 3 . The formula of nitride of element X will be (a) X 2 N (b) XN 2 (c) XN (d) X 2 N 3

Answer: (c) XN

The formula of a compound is X 3 Y. The valencies of elements X and Y will be respectively (a) 1 and 3 (b) 3 and 1 (c) 2 and 3 (d) 3 and 2

Answer: (a) 1 and 3

A mole of an atom is a collection of atoms whose total mass is the number of grams equal to the atomic mass. Since an equal number of moles of different elements contain an equal number of atoms it becomes convenient to express the amounts of the elements in terms of moles. A mole represents a definite number of particles viz, atoms, molecules, ions or electrons. This definite number is called the Avogadro number or Avogadro constant which is equal to 6.022 × 1023. Hence a mole represents 6.022 × 1023 particles of the substance. One mole of a substance represents one gram-formula of the substance. One mole of a gas at standard temperature and pressure occupies 22.4 litres.

How many grams of sodium must be taken to get 1 mole of the element? (a) 23 g (b) 35.5 g (c) 63.5 g (d) 46 g

Answer: (a) 23 g

What is the mass in grams of a single atom of chlorine? (Atomic mass of chlorine = 35.5) (a) 6.54 × 10 23 g (b) 5.9 × 10 –23 g (c) 0.0025 g (d) 35.5 g

Answer: (b) 5.9 × 10–23 g

How many number of moles are there in 5.75 g of sodium ? (Atomic mass of sodium = 23) (a) 0.25 (b) 0.5 (c) 1 (d) 2.5

Answer: (a) 0.25

What is the mass in grams of 2.42 mol of zinc? (Atomic mass of Zn = 65.41) (a) 200 g (b) 25 g (c) 85 g (d) 158 g

Answer: (d) 158 g

According to Dalton’s atomic theory, all matter whether an element, a compound, or a mixture is composed of small particles called atoms which can neither be created nor destroyed during a chemical reaction. Dalton’s theory provides a simple explanation for the laws of chemical combination. He used his theory to explain the law of conservation of masses, the law of constant proportions, and the law of multiple proportions, based on various postulates of the theory. Dalton was the first scientist to use the symbols for the elements in a very specific sense. When he used a symbol for an element he also meant a definite quantity of that element, that is one atom of that element.

Which postulate of Dalton’s atomic theory is the result of the law of conservation of mass? (a) Atoms can neither be created nor destroyed. (b) Each element is composed of extremely small particles called atoms. (c) All the atoms of a given element are identical. (d) During chemical combination, atoms of different elements combine in simple ratios.

Answer: (a) Atoms can neither be created nor destroyed.

Which postulate of Dalton’s atomic theory explains law of definite proportions? (a) Atoms of an element do not change during a chemical reaction. (b) An element consists of atoms having fixed mass and the number and kind of atoms in a given compound is fixed. (c) Different elements have different kind of atoms. (d) Atoms are of various kinds

Answer: (b) An element consists of atoms having fixed mass and the number and kind of atoms in a given compound is fixed.

“If 100 g of calcium carbonate (whether in the form of marble or chalk) is decomposed, 56 g of calcium oxide and 44 g of carbon dioxide are formed.” Which law of chemical combination is illustrated by this statement? (a) Law of constant proportions (b) Law of conservation of mass (c) Law of multiple proportions (d) Law of conservation of energy

Answer: (b) Law of conservation of mass

When 5 g calcium is burnt in 2 g oxygen, 7 g of calcium oxide is produced. When 5 g of calcium is burnt in 20 g of oxygen, then also 7 g of calcium oxide is produced. Which law of chemical combination is being followed? (a) Law of conservation of mass (b) Law of multiple proportions (c) Law of constant proportions (d) No law is being followed.

Answer: (c) Law of constant proportions

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