thermodynamics case study questions

Class 11 Chemistry Case Study Questions Chapter 6 Thermodynamics

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In Class 11 Final Exams there will be Case studies and Passage Based Questions will be asked, So practice these types of questions. Study Rate is always there to help you. Free PDF Downloads of CBSE Class 11 Chemistry Chapter 6 Case Study and Passage-Based Questions with Answers were Prepared Based on the Latest Exam Pattern. Students can solve Class 11 Chemistry Case Study Questions Thermodynamics to know their preparation level.

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In CBSE Class 11 Chemistry Paper, 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.

Thermodynamics Case Study Questions With Answers

Here, we have provided case-based/passage-based questions for Class 11 Chemistry  Chapter 6 Thermodynamics

Case Study/Passage-Based Questions

Case Study 1: Hess’s Law of Constant Heat Summation – This law was presented by Hess in 1840. According to the law, if a chemical reaction can be made to take place in a number of ways in one or in several steps, the total enthalpy change is always the same. Thus, the total enthalpy change of a chemical reaction depends on the initial and final stages only.

In which of the enlisted cases, Hess’s law is not applicable? (a) Determination of lattice energy (b) Determination of resonance energy (c) Determination of enthalpy of transformation of one allotropic form to another (d) Determination of entropy

Answer: (d) Determination of entropy

Use the bond energy data and calculate the enthalpy change for

Answer: (c) -1428kJ/mol

A hypothetical reaction, A 2B, proceeds through the following sequence of steps :

Answer: (c) q1+q2+2q3

Case Study 2: The enthalpy of a system is defined as the sum of the internal energy of the system and the energy that arises due to its pressure and volume. Mathematically, the enthalpy is defined by the equation, H = U + PV Enthalpy change (ΔH) of a system is the heat absorbed or evolved by the system at constant pressure. ΔH = qp, ΔH = ΔU + PΔV

Which of the following is not correct about enthalpy? (a) It is an extensive property. (b) It is not a state function. (c) Its absolute value cannot be determined. (d) Enthalpy of a compound is equal to the enthalpy of formation of that compound.

Answer: (b) It is not a state function.

Lattice enthalpies are determined by (a) Born-Haber cycle (b) Hess’s law (c) lattice cycle (d) none of these

Answer: (a) Born-Haber cycle

In which of the following thermochemical changes ΔH is always negative? (a) Enthalpy of solution (b) Enthalpy of hydrogenation (c) Enthalpy of reaction (d) Enthalpy of transition

Answer: (b) Enthalpy of hydrogenation

Case Study 3: Thermodynamics is a branch of chemistry that deals with the study of energy transformations in chemical and physical processes. It is concerned with the interrelation of heat and work with chemical reactions or physical changes in a system. One of the key concepts in thermodynamics is the notion of internal energy, which is the sum of the kinetic and potential energies of the particles within a system. The first law of thermodynamics, also known as the law of energy conservation, states that energy cannot be created or destroyed, only converted from one form to another. It establishes the principle of energy conservation and the concept of heat transfer as a form of energy flow. The second law of thermodynamics deals with the direction of energy flow and states that in natural processes, the total entropy of a system and its surroundings always increases. Entropy is a measure of the disorder or randomness in a system, and this law provides insights into the irreversibility of certain processes.

Thermodynamics is a branch of chemistry concerned with the study of: (a) Particle interactions (b) Energy transformations in chemical and physical processes (c) Atomic structures (d) Organic reactions

Answer: (b) Energy transformations in chemical and physical processes

Internal energy in a system is the sum of: (a) Kinetic energy of particles only (b) Potential energy of particles only (c) Both kinetic and potential energies of particles (d) Total energy of the system

Answer: (c) Both kinetic and potential energies of particles

The first law of thermodynamics is also known as the law of: (a) Heat transfer (b) Energy conservation (c) Entropy increase (d) Internal energy

Answer: (b) Energy conservation

The second law of thermodynamics states that in natural processes, the total entropy of a system and its surroundings always: (a) Decreases (b) Remains constant (c) Fluctuates (d) Increases

Answer: (d) Increases

Hope the information shed above regarding Case Study and Passage Based Questions for Class 11 Chemistry Chapter 6 Thermodynamics with Answers Pdf free download has been useful to an extent. If you have any other queries about the CBSE Class 11 Chemistry Thermodynamics 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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Class 11th Chemistry - Thermodynamics Case Study Questions and Answers 2022 - 2023

Class 11th Chemistry - Thermodynamics Case Study Questions and Answers 2022 - 2023 Study Materials Sep-09 , 2022

QB365 provides a detailed and simple solution for every Possible Case Study Questions in Class 11 Chemistry Subject - Thermodynamics, CBSE. It will help Students to get more practice questions, Students can Practice these question papers in addition to score best marks.

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Thermodynamics case study questions with answer key.

Final Semester - June 2015

Thermodynamics involve energy changes in chemical reactions and other processes. Internal energy is total energy stored in a substance. We can specify absolute value of volume but not the absolute value of internal energy. We can measure only change in internal energy ( \(\triangle\) U). Work done on the system is taken as positive and work done by the system is taken as negative. Heat (q) absorbed by the system is +ve and heat given out by system is negative. \(\triangle\) U = q + w according to first law of thermodynamics. \(\triangle\) H (enthalpy change) is measured at constant pressure, \(\triangle\) U is measured at constant volume. \(\triangle\) H, \(\triangle\) S (entropy change), \(\triangle\) G (free energy change) and temperature help to decide spontaneity of the process. (a) What is \(\triangle\) U in adiabatic process? (b) If 701 J of heat is absorbed by the system and 394 J of work is done by the system. What is value of \(\triangle\) U? (c) 2 litres of an ideal gas at a pressure of 10 atm expands isothermally into vacuum until its total volume is 10 litres. How much heat is absorbed and work done in the expansion? (d) For an equilibrium H 2 O(1)  \(\rightleftharpoons\)   H 2 O(g), What are sign of \(\triangle\) G, \(\triangle\) H and \(\triangle\) S? (e) For N 2 O 4 (g)  \(\rightleftharpoons\)   2NO 2 (g). (f) What is C p - C v  equal to? (g) State second law of thermodynamics.

Observe the table of standard enthalpy change for fusion and vapourisation of some substances. Study the table and answer the following questions. Standard Enthalpy Changes of Fusion and Vapourisation

(a) Why is \(\triangle\) H vap of NaCI highest? (b) What is \(\triangle\) s for H 2 O(s)  \(\rightarrow\)  H 2 O(I)? (c) Which has stronger intermolecular forces, CCl 4 or Acetone? (d) calculate \(\triangle\) U vap for H 2 O if \(\triangle\) H vap = 40.66 kJ mol -1 at 373 K for 1 mole. (e) NH 3 (g)  \(\rightarrow\) NH 3 (l). What is sign of \(\triangle\) s? (f) How is enthalpy of sublimation calculated? (g) What is relationship between ionisation enthalpy and ionisation energy?

We can measure the transfer of heat from one system to another which cause change in temperature. The magnitude of change in temperature depends upon heat capacity of the substance. The enthalpy change of reaction remains the same irrespective of number ofsteps is Hess's law.It helps to calculate enthalpy of formation, combustion and other enthalpy changes. Enthalpy change can also be calculated by using bond enthalpies. First law gives law of conservation of energy but does not give direction of reaction. Second law states, entropy of universe is continuously increasing due to spontaneous processes taking place in it. \(\Delta\) H and \(\Delta\) S (entropy change) cannot decide spontaneity of process. We need \(\Delta\) G (free energy change) which is -ve for spontaneous, +ve for non-spontaneous. \(\Delta\) G = 0 for process in equilibrium. \(\Delta\) G is related to equilibrium constant. If \(\Delta\) G = -ve, 'K' is +ve and vice versa. Third law of thermodynamics states the entropy of perfectly crystalline substance is zero at zero kelvin. (a) We can determine \(\Delta\) H lattice with the help of cycle. Name the cycle. (b) How can we calculate enthalpy of solution? (c) What is molar heat capacity of water in equilibrium with ice at constant pressure? (d)  \(\Delta \mathbf{H}_{f}^{\circ}\)   of O 3 , CaO, H 3  and HI are +142.2,- 643.9,-46, +25.95 kJ mol -1 . Arrange these in increasing order of stability. (e) Standard entropy of X 2 , Y 2 and XY 3 are 60, 40 and 50 JK -1 mol -1  respectively. For the reaction  \(\frac{1}{2} \mathbf{X}_{2}+\frac{3}{2} \mathbf{Y}_{2} \longrightarrow \mathbf{X Y}_{3}, \Delta \mathbf{H}=-\mathbf{3 0}\)   KJ to be at what temperature, process will be at equilibrium. (f) What are sign of \(\Delta\) H and \(\Delta\) S for process to be always spontaneous? (g) Give mathematical expression for second law of thermodynamics.

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