Thermodynamics Mock Test – Class 11 Chemistry

1. 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

2. Standard thermodynamic data are reported for substances in their standard states. The statement that best avoids a common confusion is

3. Assertion: If a thermochemical equation is reversed while applying Hess law, the sign of must be reversed.
Reason: Reversing the equation interchanges the initial and final thermodynamic states.

4. A gas is compressed from to against a constant external pressure of . During compression, of heat is released by the gas. Use . If the final pressure-volume term is smaller than the initial pressure-volume term, the enthalpy change is closest to

5. The table shows operations on a thermochemical equation with original enthalpy change .

The correctly matched entries are

6. In a standard-state thermochemical calculation involving an aqueous solute, the standard state of the solute is most commonly treated as

7. Assertion: In an adiabatic compression of a gas, can be positive.
Reason: In adiabatic compression, and work is done on the system.

8. The following pairs are listed for classification:

The pair containing only path functions is

9. A neutralization reaction is carried out in a coffee-cup calorimeter. of acid and of base are mixed, and of water is formed. The total solution mass is , , and the temperature rises by . Neglecting the cup heat capacity, the enthalpy of neutralization per mole of water formed is

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

11. A reaction has in the forward direction at a certain temperature. The equilibrium constant for the reverse reaction is

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

13. The row that correctly connects , , and is

The inconsistent row is

14. Two objects are at and . They are brought into thermal contact, and the cooler object is chosen as the system. The sign of heat for the cooler object during the initial contact is

15. Use the arrangement described below.

The most suitable prediction is

16. The table gives heat and work data for three processes of the same system.

The process with the greatest increase in internal energy is

17. The relation connecting actual Gibbs energy change, standard Gibbs energy change, and reaction quotient is

18. A student writes the following description: “For a reaction mixture taken as system, the surroundings are only the chemicals not participating in the reaction.” The best evaluation of this claim is that

19. Study the table and choose the row that misinterprets the - work graph.

20. A reaction has and . The temperature at which is

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

22. 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

23. Lattice enthalpy of an ionic solid is most closely connected with the enthalpy change when

24. A gas expands adiabatically from one state to another and its internal energy decreases by . The magnitude of work done by the gas is

25. Formation of from and has a negative enthalpy change mainly because

26. A graph of against for a reaction is a straight line with negative intercept and positive slope. The reaction has

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

28. At the normal melting point of a pure solid, solid and liquid are in equilibrium. The Gibbs energy change for melting at this temperature is

29. A container has a boundary that allows heat to pass through but does not allow the gas inside to escape. This description most strongly supports

30. The table shows four constant-volume cases for a gas.

The case with an incorrect claim is

31. A student writes, “Because , a larger always makes more positive.” The correction is that

32. Use the following standard formation enthalpies and standard molar entropies at :
, ;
, ;
, .
For , at is closest to

33. A metal sample absorbs of heat, and its temperature rises by . The specific heat capacity of the metal is

34. Enthalpy of dilution is best described as the heat change when

35. A solid sample melts at its melting point to form a liquid. The entropy change of the sample is best linked with

36. A system changes from state P to state Q by two different routes. If the initial and final states are identical in both routes, the value of will

37. A process is at equilibrium at constant and . A small change makes negative for the forward direction. The system will tend to

38. Assertion: An endothermic reaction at constant pressure has .
Reason: In an endothermic reaction, heat is absorbed by the system, and at constant pressure .

39. The table shows changes made to a reaction system at the same temperature.

The correctly matched entries are

40. For an ideal gas, is the molar heat capacity measured under the condition

41. Assertion: If and are both positive for a process, must be positive.
Reason: According to , both positive heat absorbed and positive work done on the system increase the system's internal energy.

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

43. The value of for a reaction is most directly a measure of

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

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

46. An endothermic process has and is spontaneous at high temperature but not at low temperature. The sign of must be

47. A reaction has and . Using , the forward reaction is

48. In a process, and . The work term and its meaning are

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

50. A straight-line plot of against cuts the axis at . The reaction has . The value of is