Thermodynamics Mock Test – Class 11 Chemistry

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

2. Assertion: A reversible process is an idealized process carried out through infinitesimal changes.
Reason: A reversible process is imagined to pass through states very close to equilibrium at each stage.

3. A gas expands reversibly and isothermally from to . On the - graph, the work magnitude is represented by

4. One mole of an ideal gas expands reversibly and isothermally from to . Use and . The entropy change of the gas is closest to

5. A thermodynamic state of a simple gas in a container is described most clearly by specifying measurable properties such as

6. For a reaction, standard entropy change is calculated using

7. A thermodynamic property that depends on the amount of substance present in the system is called an

8. For the change at its melting point, heat is absorbed by the system. The change is best classified as

9. A gas absorbs heat from a flame while expanding against the surroundings. For the gas taken as the system, the signs of and are

10. A reaction at has . The entropy change of the surroundings is

11. For a thermodynamic system, the absolute value of internal energy is generally not measured directly. What is normally measured and used is

12. A reaction at has and . Use and . The actual is closest to

13. Hess law is based on the fact that

14. The standard enthalpy of atomization is most closely described as the enthalpy change when

15. Consider the following statements about internal energy.
I. is a state function.
II. Only , not the absolute value of , is normally required in thermodynamic calculations.
III. depends only on the colour of the system.
The valid statements are

16. A heat interaction is recorded as for a system. This notation means that

17. 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

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

19. A gaseous reaction has , , and at . Use . The standard Gibbs energy change is closest to

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

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

22. For a reaction at , , but the current value of is very small. The forward reaction can still be spontaneous because

23. The following pairs are listed for classification:

The pair containing only path functions is

24. A process at constant pressure has . The best interpretation is that the process is

25. A reaction carried out in an insulated calorimeter causes the solution and calorimeter together to gain of heat. For the reacting system, the heat change is

26. The thermochemical equation has . The enthalpy change for formation of of from the same elements is

27. A catalyst is added to a reaction mixture at constant temperature. Its effect on and is best described as

28. A gas in a sealed vessel is heated, and its temperature rises. At the molecular level, this most directly suggests a change in

29. A real gas suddenly expands into a much larger evacuated vessel after a stopcock is opened. This process is best treated as

30. 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

31. The statement that best separates internal energy from heat is

32. A system absorbs of heat and has of work done on it. The change in internal energy is

33. An element in its standard state has , but this does not mean its entropy must be zero. The best reason is that

34. A gas in a rigid vessel absorbs of heat. Assuming only pressure-volume work is considered, the change in internal energy is

35. Use bond enthalpies , , and . For , the approximate is

36. A gas sample is enclosed by a movable piston made of a heat-conducting material. The piston fits tightly, so no gas escapes. The boundary permits

37. The electron gain enthalpy step for chlorine in the formation of is best written as

38. The expression is equivalent to the natural logarithm form because

39. A relation-selection table is shown below.

The correctly matched entries are

40. Read the situation below and answer the question.

What belongs to the surroundings in this description?

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

42. For the reaction , the sign of is expected to be

43. For the same substance at the same temperature range, the arrangement with the greatest entropy is generally

44. A system changes from state 1 to state 2. The internal energy increases by , and the term increases by . The enthalpy change is

45. A reversible isothermal expansion of ideal gas at is carried out from to . The same gas is then cooled at constant volume from to . Given , , and , the total for the two steps is closest to

46. A neutralization reaction is performed in a coffee-cup calorimeter. of acid and of base are mixed. The final solution has mass , , the calorimeter constant is , and the temperature increases from to . If of water is formed, the molar enthalpy of neutralization is closest to

47. Use the situation below.

The correct prediction is

48. The relation between enthalpy change and internal energy change for a general process is

49. Bond enthalpy is most directly associated with

50. A cyclic process has total heat absorbed by the system . Using the first-law sign convention , what is the total work for the cycle?