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Thermodynamics (Test 2)
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Thermodynamics (Test 2)
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25 Questions

1. A quantity that is zero when a reaction is at equilibrium at constant temperature and pressure
2. The decomposition of CaCO3(s) is shown in the equation above. Using the data in the table above the reaction, which of the following values is closest to the ΔHrxn of the decomposition of CaCO3(s)?
3. Given the bond energies in the table above, which of the following statements best describes the formation of 1 mole of H2O(l) from H2(g) and O2(g)?
4. The energy needed to convert an ionic solid into well-separated gaseous ions
5. Considering the data in the table above, which of the following must be true of the reaction?
6. The entropy change for the dissolution of calcium chloride in water shown above might be expected to be positive, but the actual ΔS is negative. Which of the following is the most plausible explanation for the net loss of entropy during this process?
7. The energy liberated from a physical or chemical process that is available to do work
8. The reactions for the combustion of diamond and graphite are shown above. Which of the following values is closest to the ΔHrxn for the conversion of C(graphite) to C(diamond)?
9. True for the combustion of wood into CO2(g) and H2O(g) in a campfire
10. The standard Gibbs free energy change, ΔG°298, for the conversion of Cdiamond into Cgraphite has an approximate value of –3 kJ mol−1. However, graphite does not form from diamond under standard conditions (298 K and 1 atm). Which of the following best explains this observation?
11. True for the deposition of CO2(g) into CO2(s) at –100°C and 1 atm
12. The formula for this quantity is used to derive the effusion ratio of O2 and CO2 at the given temperature
13. The energy needed for the formation of the transition state of a chemical reaction
14. Which of the following reactions involves the largest decrease in entropy?
15. A quantity that describes a feature of a chemical reaction and is always positive for reactions in which an increase in temperature results in an increased reaction rate
16. A quantity that is zero for a perfect, pure crystalline solid at 0 K
17. This quantity is determined by measuring the rate of a particular reaction at two or more different temperatures
18. Must be true for a reaction that is never spontaneous at any temperature
19. Must be true for a reaction that is spontaneous at all temperatures
20. The energy needed to overcome the activation barrier of a chemical reaction
21. True for melting of water at 25°C and 1 atm
22. The combustion of methylhydrazine, a common rocket fuel, is represented above. The ΔH of this reaction is –1,303 kJ mol−1CH6N2(l). What would be the ΔH per mol CH6N2(l) if the reaction produced H2O(l) instead of H2O(g)? (The ΔH for the condensation of H2O(g) to H2O(l) is –44 kJ mol−1.)
23. A quantity that is zero for a pure element in its standard state
24. The normal melting point of Ag(s) is 962°C. Which of the following is true for the process represented above at 962°C?
25. Which of the following processes demonstrates a decrease in entropy (ΔS < 0)?

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