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Basic Chemistry Practice Test: Chemical Thermodynamics
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Chemical thermodynamics is the study of how heat and work relate to each other in chemical reactions and physical changes of state. It also involves a set of rules and laws that explain which processes can happen spontaneously and which need some help.  The primary goal of chemical thermodynamics is to determine the feasibility of a given transformation. It is used to predict energy exchanges in the following processes: Chemical reactions Phase changes Formation of solutions  The state functions that are most important in chemical thermodynamics are: Internal energy (U) Enthalpy... Show more
Basic Chemistry Practice Test: Chemical Thermodynamics
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25 Questions

1. The value of ΔH° for the formation of POCl3 from its constituent elements, P2 (g) + O2 (g) + 3Cl2 (g) . 2POCl3 (g) is __________ kJ/mol.
2. The value of ΔG° at 25 °C for the decomposition of POCl3 into its constituent elements, 2POCl3 (g) . P2 (g) + O2 (g) + 3Cl2 (g) is __________ kJ/mol.
3. The melting of a substance at its melting point is an isothermal process.
4. Consider the reaction:
NH3 (g) + HCl (g) . NH4Cl (s) Given the following table of thermodynamic data at 298 oK:
.................. .... .... ............... .... .. ..... .. ........ .. .. .. ...... ............ .......... .. .... ...... ............ ............ .. .. ...... ...... ............ ........ The value of K for the reaction at 25 °C is __________.
5. The equilibrium constant for a reaction is 0.48 at 25 °C. What is the value of ΔG° (kJ/mol) at this temperature?
6. The value of ΔG° at 25 °C for the formation of calcium chloride from its constituent elements, Ca (s) + Cl2 (g) . CaCl2 (s) is __________ kJ/mol.
7. Which reaction produces a decrease in the entropy of the system?
8. Which one of the following is always positive when a spontaneous process occurs?
9. The value of ΔG° at 25 °C for the formation of POCl3 from its constituent elements, P2 (g) + O2 (g) + 3Cl2 (g) . 2POCl3 (g) is __________ kJ/mol.
10. Which one of the following processes produces a decrease of the entropy of the system?
11. The thermodynamic quantity that expresses the degree of disorder in a system is __________.
12. When a system is at equilibrium, __________.
13. The combustion of ethene in the presence of excess oxygen yields carbon dioxide and water:
C2H4 (g) + 3O2 (g) . 2CO2 (g) + 2H2O (l) The value of ΔS° for this reaction is __________ J/K.
14. Of the following, the entropy of __________ is the largest.
15. Which one of the following processes produces a decrease in the entropy of the system?
16. The value of ΔG° at 100.0 °C for the formation of calcium chloride from its constituent elements:
Ca (s) + Cl2 (g) . CaCl2 (s) is __________ kJ/mol. At 25.0 oC for this reaction, ΔH° is -795.8 kJ/mol, ΔG° is -748.1 kJ/mol, and ΔS° is -159.8 J/K.
17. The second law of thermodynamics states that __________.
18. The value of ΔH° for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S (s, rhombic) + O2 (g) . SO2 (g) is __________ kJ/mol.
19. The value of ΔH° for the decomposition of POCl3 into its constituent elements, 2POCl3 (g) . P2 (g) + O2 (g) + 3Cl2 (g) is __________ kJ/mol.
20. A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if .H is__________ and ΔS is __________.
21. In the Haber process, ammonia is synthesized from nitrogen and hydrogen:
N2 (g) + 3H2 (g) . 2NH3 (g) ΔG° at 298 oK for this reaction is -33.3 kJ/mol. The value of .G at 298 K for a reaction mixture that consistsof 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is __________.
22. Which one of the following statements is true about the equilibrium constant for a reaction if ΔG° for the reaction is negative?
23. Of the following, only __________ is not a state function.
24. For the reaction C(s) + H2O (g) . CO(g) + H2 (g) ΔH° = 131.3 kJ/mol and ΔS° = 133.6 J/K · mol at 298 K. At temperatures greater than __________°C this reaction is spontaneous under standard conditions.
25. The value of ΔG° at 100.0 °C for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S (s, rhombic) + O2 (g) . SO2 (g) is __________ kJ/mol. At 25.0 oC for this reaction, ΔH° is -269.9 kJ/mol, ΔG° is -300.4kJ/mol, and ΔS° is +11.6 J/K.

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