Thermodynamics Mock Test – Class 11 Chemistry

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

2. For a system that releases of heat, the same heat transfer written in joules with the correct sign is

3. A state record for a fixed amount of gas changes as follows:

The record shows that the process is

4. A sample absorbs the same heat in two trials. In Trial P, its temperature rise is . In Trial Q, its temperature rise is . The heat capacity in Trial P compared with Trial Q is

5. A reaction at has . Use and . The standard Gibbs energy change is closest to

6. For a reaction at a fixed temperature, the current mixture has . The forward direction is favoured because

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

8. The table gives four processes for a system. The process that must have is

9. 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

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

11. For a reaction, the standard enthalpy change can be calculated using formation enthalpies by

12. A body has heat capacity . If its temperature is raised from to , the heat absorbed is

13. For an ideal gas, is larger than mainly because at constant pressure

14. For , the entropy and temperature effects suggest that the decomposition is favoured more at high temperature when . The main reason is

15. A solid has and under compatible conditions. The approximate enthalpy of sublimation is

16. A reaction has and . At , is

17. The unit belongs most directly to

18. A gas expands from to into vacuum. The value of is

19. A student says, “A salt can dissolve only if its enthalpy of solution is negative.” The best correction is that

20. Hess law is based on the fact that

21. For , at . If the current reaction quotient is , use and . The actual is closest to

22. A reaction has total bond enthalpy of bonds broken and total bond enthalpy of bonds formed . The reaction is best described as

23. Average bond enthalpy values are often approximate for polyatomic molecules because

24. A chemist records the following for a gaseous mixture: , , , and composition with by amount. The inclusion of composition is necessary because

25. A non-spontaneous reaction has . It is coupled to a second reaction with . The combined process is

26. Standard enthalpy change is usually reported for substances in their standard states at a pressure of

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

28. The pair in which both quantities are forms of energy transfer in thermodynamics is

29. A route map shows three paths from the same initial state to the same final state:
Path P: slow heating followed by expansion
Path Q: expansion followed by heating
Path R: a single combined heating-expansion step
For the internal energy change, the best conclusion is

30. Match the enthalpy term with the most suitable description.

31. A compound is burned in a bomb calorimeter. The calorimeter heat capacity is , the temperature rise is , and of the compound burns. For the reaction, at . Use . The molar enthalpy change of combustion is closest to

32. Heat transfer between two bodies occurs naturally because of

33. A ideal gas sample is heated by . If and , the constant-pressure heat absorbed is closest to

34. At constant temperature and pressure, the condition for a spontaneous process is

35. A reaction mixture in a flask is selected for thermodynamic study. The air, table, and room outside the flask are mainly part of the

36. In free expansion of a gas into vacuum, the external pressure opposing expansion is

37. A claim says, “If work is done in a process, the system must also exchange matter.” The best evaluation is that the claim is

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

39. A reaction has at a certain temperature. A mixture is prepared with . The sign of for the forward reaction is

40. A reaction has at its current composition but . The equilibrium constant at that temperature must be

41. Use the arrangement described below.

The most suitable prediction is

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

43. The table gives bond-count information for a reaction.

The row with the incorrect interpretation is

44. Use bond enthalpies , , , and . For , estimate by counting only bonds that change.

45. For the reaction , . The standard enthalpy of formation of is

46. For the same substance under comparable conditions, entropy is generally greatest in the gaseous state because

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

48. Study the classification table and identify the row that is not consistent with the usual extensive-intensive distinction.

49. A gas expands from to . In Process P, it expands against . In Process Q, it expands against . Use . The difference in work magnitudes is

50. The following pairs are listed for classification:

The pair containing only path functions is