1. © 2015 Pearson Education, Inc. Clicker Questions Chapter 19 Barbara Mowery York College

2. © 2015 Pearson Education, Inc. Which process is not spontaneous at 25 degrees Celsius? a.the melting of an ice cube b.the sublimation of dry ice c.the boiling of liquid nitrogen d.the freezing of ethyl alcohol

3. © 2015 Pearson Education, Inc. Which process is not spontaneous at 25 degrees Celsius? a.the melting of an ice cube b.the sublimation of dry ice c.the boiling of liquid nitrogen d.the freezing of ethyl alcohol

4. © 2015 Pearson Education, Inc. All spontaneous processes are a.reversible. b.isothermal. c.irreversible. d. exothermic.

5. © 2015 Pearson Education, Inc. All spontaneous processes are a.reversible. b.isothermal. c.irreversible. d. exothermic.

6. © 2015 Pearson Education, Inc. Entropy is a measurement of the _______ of a system. a.randomness b.internal energy c.temperature d.polarity

7. © 2015 Pearson Education, Inc. Entropy is a measurement of the _______ of a system. a.randomness b.internal energy c.temperature d.polarity

8. © 2015 Pearson Education, Inc. Entropy (S) is a state function, so the change in entropy is given by S final _____ S initial. a.+ b.− c.× d. /

9. © 2015 Pearson Education, Inc. Entropy (S) is a state function, so the change in entropy is given by S final _____ S initial. a.+ b.− c.× d. /

10. © 2015 Pearson Education, Inc. The entropy of a sample of CO 2 increases upon heating because all three types of molecular motion increase. a.True b.False

11. © 2015 Pearson Education, Inc. The entropy of a sample of CO 2 increases upon heating because all three types of molecular motion increase. a.True b.False

12. © 2015 Pearson Education, Inc. The entropy of a sample of Ne increases upon heating because all three types of molecular motion increase. a.True b.False

13. © 2015 Pearson Education, Inc. The entropy of a sample of Ne increases upon heating because all three types of molecular motion increase. a.True b.False

14. © 2015 Pearson Education, Inc. The Second Law of Thermodynamics says that the entropy of the universe _______ whenever a spontaneous process occurs. a.increases b.decreases c.remains unchanged d. reaches equilibrium

15. © 2015 Pearson Education, Inc. The Second Law of Thermodynamics says that the entropy of the universe _______ whenever a spontaneous process occurs. a.increases b.decreases c.remains unchanged d. reaches equilibrium

16. © 2015 Pearson Education, Inc. An automobile being driven from west to east is experiencing _______ motion. a.kinetic b.rotational c.vibrational d.translational

17. © 2015 Pearson Education, Inc. An automobile being driven from west to east is experiencing _______ motion. a.kinetic b.rotational c.vibrational d.translational

18. © 2015 Pearson Education, Inc. Changes in a molecule’s bond lengths or bond angles are examples of _______ motion. a.kinetic b.rotational c.vibrational d.translational

19. © 2015 Pearson Education, Inc. Changes in a molecule’s bond lengths or bond angles are examples of _______ motion. a.kinetic b.rotational c.vibrational d.translational

20. © 2015 Pearson Education, Inc. When a molecule spins like a top, it is undergoing _______ motion. a.kinetic b.vibrational c.translational d.rotational

21. © 2015 Pearson Education, Inc. When a molecule spins like a top, it is undergoing _______ motion. a.kinetic b.vibrational c.translational d.rotational

22. © 2015 Pearson Education, Inc. k = Boltzmann constant. W = the number of microstates. S = entropy. Which is true? a.S = k × W b.S = k / W c.S = k ln W d. S = k W

23. © 2015 Pearson Education, Inc. k = Boltzmann constant. W = the number of microstates. S = entropy. Which is true? a.S = k × W b.S = k / W c.S = k ln W d. S = k W

24. © 2015 Pearson Education, Inc. Entropy decreases when a.a liquid becomes a gas. b.a solid becomes a liquid. c.a gas becomes a solid. d.the number of moles of gas increases.

25. © 2015 Pearson Education, Inc. Entropy decreases when a.a liquid becomes a gas. b.a solid becomes a liquid. c.a gas becomes a solid. d.the number of moles of gas increases.

26. © 2015 Pearson Education, Inc. Which process does not illustrate a decrease in entropy? a.Na(s) + Br 2 (l)  2 NaBr(s) b.CaCO 3 (s)  CaO(s) + CO 2 (g) c.NH 3 (aq) +H 2 S(g)  (NH 4 ) 2 S(aq) d.AgNO 3 (aq) + KCl(aq)  AgCl(s) + KNO 3 (aq)

27. © 2015 Pearson Education, Inc. Which process does not illustrate a decrease in entropy? a.Na(s) + Br 2 (l)  2 NaBr(s) b.CaCO 3 (s)  CaO(s) + CO 2 (g) c.NH 3 (aq) +H 2 S(g)  (NH 4 ) 2 S(aq) d.AgNO 3 (aq) + KCl(aq)  AgCl(s) + KNO 3 (aq)

28. © 2015 Pearson Education, Inc. The Third Law of Thermodynamics says that the entropy of a pure, perfect crystal is _______ at absolute zero (zero Kelvins). a.increasingb. decreasing c. infinited. zero

29. © 2015 Pearson Education, Inc. The Third Law of Thermodynamics says that the entropy of a pure, perfect crystal is _______ at absolute zero (zero Kelvins). a.increasingb. decreasing c. infinited. zero

30. © 2015 Pearson Education, Inc. The notation, pressure, temperature, and units for reporting Standard Molar Entropies are a.S std ; 1 atm; 0° C; kJ/mol-°C. b.S°; 1 atm; 298 K; J/mol-K. c.ΔS°; 0 atm; 298 K; J/mol-K. d.ΔS° f ; 1 atm; 0° C; kJ/°C.

31. © 2015 Pearson Education, Inc. The notation, pressure, temperature, and units for reporting Standard Molar Entropies are a.S std ; 1 atm; 0° C; kJ/mol-°C. b.S°; 1 atm; 298 K; J/mol-K. c.ΔS°; 0 atm; 298 K; J/mol-K. d.ΔS° f ; 1 atm; 0° C; kJ/°C.

32. © 2015 Pearson Education, Inc. Which is not a standard condition for reporting Standard Free Energy values? a. is 0 for pure liquids and solids, regardless of their state. b. is reported for solutions at 1 M. c. is reported for gases at 1 atm. d. is 0 for pure elements in their standard states.

33. © 2015 Pearson Education, Inc. Which is not a standard condition for reporting Standard Free Energy values? a. is 0 for pure liquids and solids, regardless of their state. b. is reported for solutions at 1 M. c. is reported for gases at 1 atm. d. is 0 for pure elements in their standard states.

34. © 2015 Pearson Education, Inc. G = the Gibbs free energy. H = enthalpy. S = entropy. T = the Kelvin temperature. Which is true? a.G = H + TS b.G = H − TS c.G = H × TS d.G = H / TS

35. © 2015 Pearson Education, Inc. G = the Gibbs free energy. H = enthalpy. S = entropy. T = the Kelvin temperature. Which is true? a.G = H + TS b.G = H − TS c.G = H × TS d.G = H / TS

36. © 2015 Pearson Education, Inc. If the enthalpy change is positive and the entropy change is negative, the reaction is a.spontaneous at all temperatures. b.non-spontaneous at all temperatures. c.spontaneous at low temperatures. d.spontaneous at high temperatures.

37. © 2015 Pearson Education, Inc. If the enthalpy change is positive and the entropy change is negative, the reaction is a.spontaneous at all temperatures. b.non-spontaneous at all temperatures. c.spontaneous at low temperatures. d.spontaneous at high temperatures.

38. © 2015 Pearson Education, Inc. If the enthalpy change is negative and the entropy change is positive, the reaction is a.spontaneous at all temperatures. b.non-spontaneous at all temperatures. c.spontaneous at low temperatures. d. spontaneous at high temperatures.

39. © 2015 Pearson Education, Inc. If the enthalpy change is negative and the entropy change is positive, the reaction is a.spontaneous at all temperatures. b.non-spontaneous at all temperatures. c.spontaneous at low temperatures. d. spontaneous at high temperatures.

40. © 2015 Pearson Education, Inc. At equilibrium, the value of the free energy change (“delta G”) is a.positive. b.negative. c.fluctuating. d. zero.

41. © 2015 Pearson Education, Inc. At equilibrium, the value of the free energy change (“delta G”) is a.positive. b.negative. c.fluctuating. d. zero.

42. © 2015 Pearson Education, Inc. The general equation used to calculate ΔG rxn from standard free energies of formation is ΔG rxn = a.ΔH rxn − T ΔS rxn. b.Σn(ΔG f ) products −Σ n(ΔG f ) reactants. c.Σn(ΔG f ) reactants −Σ n(ΔG f ) products. d. ΔG f − RT lnQ.

43. © 2015 Pearson Education, Inc. The general equation used to calculate ΔG rxn from standard free energies of formation is ΔG rxn = a.ΔH rxn − T ΔS rxn. b.Σn(ΔG f ) products −Σ n(ΔG f ) reactants. c.Σn(ΔG f ) reactants −Σ n(ΔG f ) products. d. ΔG f − RT lnQ.