11th Class Chemistry Unit 6 Chemical Energetics MCQs

1.Which of the following equations represents standard heat of formation of C2H4?

2.Which of the following equations correctly defines lattice energy of MgCl2?

3.Suppose there are 100 molecules of a gas initially in jar A, which is connected to an evacuated jar B. When the stopcock is opened, the possible ways of arrangement of molecules will be:

4.For a reaction to occur spontaneously,

5.The caloric content of food, often expressed in Calories (kcal), is fundamentally related to which thermodynamic quantity during its metabolism or combustion?

6.Which of the following quantities is NOT typically determined using Hess's Law?

7.Which of the following factors would lead to a greater enthalpy change of hydration (more exothermic)?

8.The enthalpy of solution can be expressed in terms of which of the following enthalpy changes?

9.Which of the following reactions has an enthalpy change that is equal to the standard enthalpy of formation of water, ΔH°f(H2O)?

10.The enthalpy change for a reaction depends on:

11.Which of the following processes would typically result in an increase in entropy of the system?

12.Consider a reaction with ΔH>0 and ΔS<0. This reaction will be:

13.Which of the following is always negative in an exothermic reaction?

14.The enthalpy changes when one mole of a substance burns completely in oxygen is called:

15.ΔH for an endothermic reaction is:

16.The SI unit of enthalpy is:

17.Which law states that enthalpy change is independent of the path taken?

18.The system that exchanges heat but not mass:

19.When a bond is formed:

20.The sign of ΔH during melting is:

21.Enthalpy change of a process is measured under:

22.An endothermic reaction is spontaneous when:

23.The change in internal energy is zero in:

24.Enthalpy of neutralization of strong acid and strong base is approximately:

25.The standard enthalpy of formation of elements in their standard state is:

26.Which of the following is a state function?

27.Standard conditions include all except:

28.The standard enthalpy of atomization of an element is always:

29.The enthalpy of solution is:

30.A reaction is spontaneous when:

31.If a chemical reaction has ΔH = -100 kJ/mol, it is:

32.The enthalpy of sublimation involves:

33.The enthalpy change when one mole of ionic compound is dissolved in water is:

34.Which of the following is an extensive property?

35.Enthalpy of fusion is the heat required to:

36.Which reaction releases more energy?

37.ΔH° of H2(g) is:

38.Standard enthalpy change refers to:

39.Which gas has highest molar enthalpy of combustion?

40.Energy stored in chemical bonds is:

41.Which of the following affects bond energy?

42.Which of the following has the highest bond energy?

43.The energy required to break a chemical bond is called:

44.The equation q = mcΔT is used to find:

45.Which of the following is used to measure heat changes?

46.Which of the following has maximum heat capacity?

47.Specific heat capacity is amount of heat needed to raise temp of:

48.Heat of combustion of H2 is used to determine:

49.ΔH = q at constant:

50.Enthalpy change in hydration depends on:

51.In an exothermic reaction, the energy of products is:

52.The term "lattice energy" is applicable to:

53.A negative lattice energy implies:

54.Which factor affects lattice energy?

55.The unit of lattice energy is:

56.Born-Haber cycle is used to calculate:

57.Which step in the Born-Haber cycle is always endothermic?

58.What type of reaction has a negative ΔH and ΔS?

59.Which of the following causes entropy to increase?

60.ΔH is negative and ΔS is positive. Then reaction is:

61.A process with increase in entropy and enthalpy is spontaneous at:

62.An increase in entropy favors:

63.Which is not a path function?

64.ΔG = 0 indicates:

65.A reaction is feasible if:

Unit 6: Unit 6: Chemical Energetics — Mcqs