Thermodynamics Mock Test – Class 11 Chemistry

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

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

3. An ideal gas undergoes free expansion into vacuum inside an insulated container. For the gas, , , and , but the entropy change of the gas is positive. The best explanation is that

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

5. A process has and . The process is

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

7. A student obtains a positive value for lattice enthalpy while using the formation convention. The most likely interpretation is that

8. A process has and . It becomes spontaneous only when

9. A calorimeter has . Its temperature rises by during a reaction. The heat absorbed by the calorimeter is

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

11. 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.

12. A complete thermodynamic feasibility statement for a reaction at constant temperature and pressure should include the idea that

13. The change in Gibbs energy at constant temperature is given by

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

15. A claim says, “Every sealed container is an isolated system.” The best response is that the claim

16. A learner claims, “Every exothermic reaction is spontaneous because .” The best correction is that

17. Match the process condition with its defining feature.

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

19. If dissolution of a salt in water is endothermic, the most suitable conclusion is that

20. A gas expands from to against a constant external pressure of . Use . The graph area method gives the work as

21. Entropy is best understood as a thermodynamic state function related to

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

23. A graph of against for reversible isothermal expansion of an ideal gas is a downward curve. The curve falls as increases because

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

25. The universe in a thermodynamic description is represented as

26. For a fixed positive external pressure, the sign of becomes positive when

27. The standard Gibbs energy change for a reaction can be calculated from standard enthalpy and entropy changes using

28. A gas expands from to in two ways.
Case 1: against external pressure.
Case 2: into vacuum.
Use . The work values for Case 1 and Case 2 are

29. Use the arrangement described below.

For the gas as system, the most suitable interpretation is

30. Use the graph description below.

The reaction represented by the graph is

31. A state of a system cannot be described fully by saying only “the system was heated for ” because this statement gives mainly

32. In many Born-Haber calculations for , the electron gain enthalpy of chlorine is negative. This means

33. 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

34. A reaction has and . The reaction is non-spontaneous at but spontaneous at . This observation is consistent because

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

36. Gibbs energy is related to enthalpy and entropy by

37. A reaction in a calorimeter warms both the solution and the calorimeter. The solution absorbs , and the calorimeter absorbs . For the reacting system, the heat change is

38. A process takes a system from state to state by Path 1, and another process returns it from state to state by Path 2. The net change in entropy for the complete closed path is

39. One mole of an ideal gas is heated by . The difference between heat required at constant pressure and heat required at constant volume is closest to

40. At constant temperature and pressure, the entropy change of the surroundings for heat exchange with a system is commonly written as

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

42. Use bond enthalpies , , , and . For , one bond and one bond are broken, while one bond and one bond are formed. The approximate is

43. The row that correctly distinguishes thermodynamic spontaneity from rate is

The correct evaluation set is

44. One mole of an ideal gas expands isothermally at from to . Path P is reversible. Path Q is irreversible against a constant external pressure of . Use , , and . The comparison of work values is

45. A reaction has and . At the temperature where , the reaction is written in reverse and then multiplied by . The , , and for the final written reaction are

46. A rigid steel vessel contains a gas and is heated from outside. If the vessel does not expand, the boundary condition mainly prevents

47. For the reaction , the reaction quotient in terms of partial pressures is

48. Heat transfer between two bodies occurs naturally because of

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

50. The following data are given at :

The correct order of equilibrium constants is