Thermodynamics Mock Test – Class 11 Chemistry

1. Study the table and identify the inconsistent row for ideal-gas heat capacities.

2. The classification of a system is based on the exchange of matter and energy across its boundary. The matching that represents the usual classification is

3. For a substance under compatible conditions, the enthalpy of sublimation is often related to fusion and vaporization by

4. A reversible phase change has at . A reaction using this vaporization step also has and at . The total for the combined process is closest to

5. A process has and . The internal energy change is

6. A reaction is spontaneous under standard conditions at , and is greater than . The most consistent statement is

7. Thermodynamics mainly deals with the study of changes involving heat, work, energy, and matter. In chemistry, its use is most directly seen when we study

8. For , use , , , and . The heat released per gram of ethanol is closest to

9. For a reaction at , the values are and . The standard Gibbs energy change is

10. In a non-standard reaction mixture, , but . This means the mixture is

11. An ionic compound forms from and with lattice formation enthalpy . The hydration enthalpies are and . The enthalpy of solution of is closest to

12. Standard Gibbs energy change refers to the Gibbs energy change when

13. A claim says, “Specific heat capacity and molar heat capacity have the same unit because both measure heat needed for temperature rise.” The best correction is that

14. A process has , but it appears very slow at room temperature. The best conclusion is that

15. At constant volume, the first law becomes

16. One mole of ideal gas expands reversibly and isothermally at until its volume doubles. Use and . The magnitude of work is closest to

17. The term that best describes a boundary through which heat cannot pass is

18. A system releases of heat but has of work done on it. The system's internal energy

19. A reaction has at . The reaction is then written in the reverse direction and all coefficients are divided by . The new equilibrium constant is closest to

20. A cold metal block is placed in warm water. For the metal block chosen as the system, the sign of during the initial warming of the block is

21. Study the table and choose the condition under which the measured heat is directly equal to .

22. Use the following formation enthalpies:
,
,
,
.
For , is

23. A Born-Haber type energy cycle for an ionic solid is mainly an application of

24. A wall is described as permeable and diathermic. This means the wall allows

25. A reversible reaction is at equilibrium in a closed vessel. Adding more reactant suddenly changes the reaction quotient so that . Thermodynamically, the system tends to

26. A property whose change depends only on the initial and final states of a system, and not on the route followed, is called a

27. A gas absorbs of heat while expanding from to against . For the same process, at . Use and . The values of and are closest to

28. For a reaction at , and . Use . The value of is closest to

29. A reaction has and . The standard Gibbs energy change is negative

30. One mole of an ideal gas expands reversibly and isothermally at from to . Use and . For the gas, the values of , , and are closest to

31. A cup of tea cools on a table. From a thermodynamic point of view, the most suitable description is that

32. A well-stoppered thermos flask is often used as an approximate example of an isolated system because it is designed to reduce

33. A reaction has , , and . At , the actual is

34. For the reaction , the value of is

35. A reaction has at . It is coupled to a second reaction with at the same temperature. Use and . The standard Gibbs energy change of the coupled reaction is closest to

36. For , the number of gaseous moles decreases from to . The entropy change of the system is expected to be

37. At , a reaction has . Use . The equilibrium constant is closest to

38. The enthalpy of fusion of a substance is , and its melting point is . The entropy of fusion is

39. In a reaction mixture at thermodynamic equilibrium, the macroscopic properties are best described as

40. A process has and . The temperature at which is

41. A reaction has at a given temperature. The sign of is

42. In a rigid bomb calorimeter, the calorimeter absorbs of heat from a combustion reaction. For the reacting system, the internal energy change is

43. Burning of in oxygen is an important thermodynamic example because it

44. The reaction represents a standard enthalpy of formation equation because

45. A gas is enclosed in a cylinder fitted with a frictionless movable piston. The piston prevents gas from escaping, but it can move when the gas expands or contracts. The gas is best described as

46. Use the following standard formation enthalpies:
,
,
.
For , is

47. For the pair and , the lattice enthalpy magnitude is expected to be larger for because

48. A reaction has and . At , the reaction mixture has . Use and . The actual is closest to

49. A water sample is heated from to . Take . The heat absorbed is

50. A bomb calorimeter works at nearly constant volume. The heat measured in it is directly related to