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Class 11 Chemistry MCQ Chapter 6 Thermodynamics
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Thermodynamics
Chapter: 6
| MCQ |
1. What is a system in thermodynamics?
(i) The entire universe.
(ii) The part of the universe where observations are made.
(iii) The surroundings of the universe.
(iv) None of the above.
Ans: (ii) The part of the universe where observations are made.
2. Which of the following is NOT a state variable?
(i) Pressure (p).
(ii) Volume (V).
(iii) Temperature (T).
(iv) The history of the system’s changes.
Ans: (iv) The history of the system’s changes.
3. One mole of which of the following has the highest entropy?
(i) Liquid Nitrogen.
(ii) Hydrogen Gas.
(iii) Mercury.
(iv) Diamond.
Ans: (ii) Hydrogen Gas.
4. Which properties are typically used to describe a thermodynamic system?
(i) Pressure (p), temperature (T), and composition.
(ii) Position and velocity of each particle.
(iii) Mass and density only.
(iv) Temperature and humidity.
Ans: (i) Pressure (p), temperature (T), and composition.
5. A ___________in thermodynamics refers to that part of universe in which observations are made and remaining universe constitutes the ___________
(i) System, boundary.
(ii) System, surroundings.
(iii) Surroundings, system.
(iv) System, surroundings.
Ans: (ii) System, surroundings.
6. Which of the following statements is not true regarding the laws of thermodynamics ?
(i) It deal with energy changes of microscopic systems
(ii) It does not depends on the rate at which these energy transformations are carried out.
(iii) It depends on initial and final states of a system undergoing the change.
(iv) It deal with energy changes of macroscopic systems.
Ans: (i) It deal with energy changes of microscopic systems.
7. According to IUPAC conventions, when is work done on the system considered positive?
(i) When the system loses energy.
(ii) When the internal energy of the system increases.
(iii) When the system does work on the surroundings.
(iv) When the system is at equilibrium.
Ans: (ii) When the internal energy of the system increases.
8. Which of the following statements is correct?
(i) The presence of reacting species in a covered beaker is an example of open system.
(ii) The presence of reactants in a closed vessel made up of copper is an example of a closed system.
(iii) There is an exchange of energy as well as matter between the system and the surroundings in a closed system.
(iv) The presence of reactants in a thermos flask or any other closed
Ans: (ii) The presence of reactants in a closed vessel made up of copper is an example of a closed system.
9. What happens to the change in internal energy (ΔU) when there is no heat transfer or work done?
(i) ΔU becomes infinite
(ii) ΔU is positive
(iii) ΔU = 0
(iv) ΔU is negative
Ans: (iii) ΔU = 0
10. Thermodynamics is not concerned about
(i) Energy changes involved in a chemical reaction.
(ii) The extent to which a chemical reaction proceeds.
(ii) The rate at which a reaction proceeds.
(iv) The feasibility of a chemical reaction.
Ans. (iii) The rate at which a reaction proceeds.
11. What is the equation representing the change in internal energy?
(i) ΔU = q + w.
(ii) ΔU = q – w.
(iii) ΔU = w – q.
(iv) ΔU = q × w.
Ans: (i) ΔU = q + w.
12. If w = 0 and q = 0 in an isolated system, what can we say about the internal energy?
(i) It increases.
(ii) It decreases.
(iii) It remains constant.
(iv) It becomes negative.
Ans: (iii) It remains constant.
13. What happens to the enthalpy (H) when heat is absorbed by the system at constant pressure?
(i) H decreases.
(ii) H remains constant.
(iii) H increases.
(iv) H becomes negative.
Ams: (iii) H increases.
14. When chemical reactions occur at constant atmospheric pressure, which equation represents the change in internal energy?
(i) ΔU = qp + pΔV
(ii) ΔU = qp – pΔV
(iii) ΔU = qp – ΔV
(iv) ΔU = -qp + pΔV
Ans: (ii) ΔU = qp – pΔV
15. The state a gas can be described by quoting the relationship between
(i) Pressure, volume, temperature.
(ii) Temperature, amount, pressure.
(iii) Amount, volume, temperature.
(iv) Pressure, volume, temperature, amount.
