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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. What role did Karl Bosch play in development of the Haber-Bosch process?
2. A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine:
2HI (g) H2(g) + I2(g) When the system comes to equilibrium at 425 °C, PHI = 0.708 atm, and PH2 = PI2 = 0.0960 atm . The value of Kp at this temperature is __________.
3. 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)
4. 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 __________.
5. Le Chatelier's principle states that if a system at equilibrium is disturbed, the equilibrium will shift to minimizethe disturbance.
6. 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 .
7. Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) 2NO (g) + Br2 (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2 . At equilibrium the flask contained 0.46 mol of NOBr. How many moles of NO and Br2 , respectively, are in the flask at equilibrium?
8. At equilibrium, __________.
9. 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.
10. In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.
11. The equilibrium-constant expression depends on the __________ of the reaction.
12. 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.
13. 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.
14. 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?
15. 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)
16. The Keq for the equilibrium below is 7.52 × 10-2 at 480 °C. 2Cl2 (g) + 2H2O (g) 4HCl (g) + O2 (g) What is the value of Keq at this temperature for the following reaction? 4HCl (g) + O2 (g) 2Cl2 (g) + 2H2O (g)
17. 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.
18. Of the following equilibria, only __________ will shift to the left in response to a decrease in volume.
19. Consider the following equilibrium. 2 SO2 (g) + O2 (g) 2 S O3 (g) The equilibrium cannot be established when __________ is/are placed in a 1.0-L container.
20. 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 __________.
21. Consider the following reaction at equilibrium:
2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Chätelier's principle predicts that adding O2 (g) to the reaction container will __________.
22. 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?
23. 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 __________.
24. The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is Keq = __________.
25. The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of mass action.

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