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Basic Chemistry Practice Test: Chemical Equilibrium
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Avg score: 74% • Most missed: “Le Chatelier's principle states that if a system at equilibrium is disturbed, th…”
Chemical equilibrium is a state in which the concentrations of reactants and products in a chemical reaction do not change over time. This state is also known as dynamic equilibrium.  Here are some characteristics of chemical equilibrium: Forward and backward reactions: In a reversible reaction, the forward and backward reactions occur at the same speed. Constancy: At equilibrium, certain properties like concentration, density, pressure, and color remain constant. Fixed concentrations: At equilibrium, each reactant and product has a fixed concentration. Equilibrium constant: The ratio of... Show more
Basic Chemistry Practice Test: Chemical Equilibrium
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25 Questions

1. In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process forsynthesizing ammonia directly from nitrogen and hydrogen?
2. The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is Keq = __________.
3. The effect of a catalyst on a chemical reaction is to react with product, effectively removing it and shifting the equilibrium to the right.
4. Consider the following reaction at equilibrium:
2NH3 (g) N2 (g) + 3H2 (g) ΔH° = +92.4 kJ Le Chätelier's principle predicts that adding N2 (g) to the system at equilibrium will result in __________.
5. The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) is 794 at 25 °C. At this temperature, what is the value of Keq for the equilibriumbelow?
HI (g) 1/2 H2 (g) + 1/2 I2 (g)
6. The reaction below is exothermic:
2SO2 (g) + O2 (g) 2SO3 (g) Le Chätelier's Principle predicts that __________ will result in an increase in the number of moles of SO3 (g) in the reaction container.
7. For the endothermic reaction CaCO3 (s) CaO (s) + CO2 (g) Le Chätelier's principle predicts that __________ will result in an increase in the number of moles of CO2 .
8. In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction:
CO (g) + H2O (g) CO2 (g) + H2 (g)
In an experiment, 0.35 mol of CO and 0.40 mol of H2O were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.19 mol of CO remaining. Keq at the temperature of the experiment is __________.
9. At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.
10. Dinitrogentetraoxide partially decomposes according to the following equilibrium:
N2O4 (g) . 2NO2 (g) A 1.000-L flask is charged with 3.00 × 10-2 mol of N2O4 . At equilibrium, 2.36 × 10-2 mol of N2O4 remains. Keq for this reaction is __________.
11. Which one of the following will change the value of an equilibrium constant?
12. The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121:
PCl5 (g) PCl3 (g) + Cl2 (g) A vessel is charged with PCl5 , giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3 is__________ atm.
13. At 1000 K, the equilibrium constant for the reaction 2NO (g) + Br2 (g) 2NOBr (g) is Kp = 0.013. Calculate Kp for the reverse reaction, 2NOBr (g) 2NO (g) + Br2 (g).
14. The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is __________. (1) SO2 (g) + (1/2) O2 (g) SO3 (g) (2) 2SO3 (g) 2SO2 (g) + O2 (g)
15. How is the reaction quotient used to determine whether a system is at equilibrium?
16. The equilibrium-constant expression depends on the __________ of the reaction.
17. Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Chätelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________.
18. Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction:
PCl3 (g) + Cl2 (g) . PCl5 (g) An equilibrium mixture at 450 K contains PCl3 P = 0.202 atm, Cl2 P = 0.256 atm, and PCl5 P = 3.45 atm. What is the value of Kp at this temperature?
19. Dinitrogentetraoxide partially decomposes according to the following equilibrium:
N2O4 (g) 2NO2 (g) A 1.00-L flask is charged with 0.400 mol of N2O4 . At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is __________.
20. How does the reaction quotient of a reaction (Q) differ from the equilibrium constant (Keq) of the same reaction?
21. The value of Keq for the following reaction is 0.25:
SO2 (g) + NO2 (g) SO3 (g) + NO (g) The value of Keq at the same temperature for the reaction below is __________. 2SO2 (g) + 2NO2 (g) 2SO3 (g) + 2NO (g)
22. At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103. 2NO (g) N2 (g) + O2 (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is __________ atm.
23. In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Chätelier's principle?
24. Consider the following reaction at equilibrium:
2NH3 (g) N2 (g) + 3H2 (g) Le Chätelier's principle predicts that the moles of H2 in the reaction container will increase with __________
25. At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) 2BrCl (g) is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true.

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