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Basic Chemistry Practice Test: Chemical Equilibrium
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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. 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 __________.
2. The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is Keq = __________.
3. Consider the following reaction at equilibrium:
2C O2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Chätelier's principle predicts that an increase in temperature will __________.
4. Of the following equilibria, only __________ will shift to the left in response to a decrease in volume.
5. 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 __________
6. Which one of the following is true concerning the Haber process?
7. The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) is 794 at 25 °C. What is the value of Keq for the equilibriumbelow?
1/2 H2 (g) + 1/2 I2 (g) HI (g)
8. 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)
9. 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 .
10. 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)
11. A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2 . An equilibrium reaction ensues:
I2 (g) + Br2 (g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is __________.
12. 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?
13. Consider the following reaction at equilibrium:
2SO2 (g) + O2 (g) 2SO3 (g) ΔH° = -99 kJ Le Chätelier's principle predicts that an increase in temperature will result in __________.
14. At 22 °C, Kp = 0.070 for the equilibrium:
NH4HS (s) NH3 (g) + H2S (g) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains.
15. 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).
16. Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution:
HC2H3O2 (aq) C2H3O2- (aq) + H+ (aq) At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations:
[HC2H3O2 ] = 0.0990 M, -3 [C2H3O2 -] = 1.33 × 10 M and [H+ ] = 1.33 × 10-3 M. The equilibrium constant, Keq, for the ionization of acetic acid at 25 °C is __________.
17. 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.
18. TheKp for the reaction below is 1.49 × 108 at 100 °C:
CO (g) + Cl2 (g) . COCl2 (g)
In an equilibrium mixture of the three gases, PCO = Cl2 P = 8.60 × 10-4 atm. The partial pressure of the product, phosgene (COCl2 ) , is __________ atm.
19. 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.
20. 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)
21. At equilibrium, __________.
22. The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of mass action.
23. Consider the following chemical reaction:
H2 (g) + I2 (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H2 , I2 , and HI were 0.15 M, 0.033 M, and 0.55 M respectively. The value of Keq for this reaction is __________.
24. The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) is 54.0 at 427 °C. What is the value of Keq for the equilibriumbelow?
HI (g) 1/2 H2 (g) + 1/2 I2 (g)
25. 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 __________.

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