Home > Chemistry > Quizzes > Basic Chemistry Practice Test: Chemical Equilibrium
Basic Chemistry Practice Test: Chemical Equilibrium
Fast practice, instant feedback. Timer auto-submits when time’s up.
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
Time left 00:00
25 Questions

1. 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?
2. At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide:
H2 (g) + Br2 (g) 2HBr (g) A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.566 mol of H2 present. At equilibrium, there are __________ mol of Br2 present in the reaction vessel.
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. Of the following equilibria, only __________ will shift to the left in response to a decrease in volume.
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. 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?
7. The equilibrium constant for the gas phase reaction 2NH3 (g) N2 (g) + 3H2 (g) is Keq = 230 at 300 °C. At equilibrium, __________.
8. 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.
9. 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 __________.
10. 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 __________.
11. At equilibrium, __________.
12. How is the reaction quotient used to determine whether a system is at equilibrium?
13. The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g) 2NH3 (g) is Keq = 4.34 × 10-3 at 300 °C. At equilibrium, __________.
14. 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 __________.
15. The equilibrium-constant expression depends on the __________ of the reaction.
16. 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)
17. 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.
18. 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 __________
19. 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).
20. At 900 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g) . 2SO3 (g) At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is__________ atm.
21. Which one of the following will change the value of an equilibrium constant?
22. Which one of the following is true concerning the Haber process?
23. The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for the process is Keq = __________.
24. How does the reaction quotient of a reaction (Q) differ from the equilibrium constant (Keq) of the same reaction?
25. 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.

⚡ Recently practiced quizzes in this topic
Live quiz activity
Basic Chemistry Practice Test: Chemistry of the Nonmetals Chemistry Certification Basic Chemistry Basic Chemistry Practice Test: Aqueous Reactions and Solution Stoichiometry Basic Chemistry Practice Test: Organic and Biological Chemistry Basic Chemistry Practice Test: Matter and Measurement Basics Basic Chemistry Practice Test: Stoichiometry & Calculations with Equations Basic Chemistry Practice Test: Thermochemistry Basic Chemistry Practice Test: Basic Concepts of Chemical Bonding Basic Chemistry Practice Test: Modern Materials
 
❤ If you liked Fatskills, consider supporting us by checking out The Life Manuals You Never Got.

🌈  Our mission is to help improve your scores in any subject and exam withonline quizzes, practice tests, study guides, & advice for students. Since 2018.
About | Explore | User Guide | Topics | Subjects | Doubt Solver | Career Aptitude Test | Answers | Free Tools | OSHA Basics Quiz | What Should We Know?
Privacy | Terms |
Without work one finishes nothing. - Ralph Waldo Emerson
© 2026 Fatskills.com

All trademarks, logos and brand names are the property of their respective owners. All company, product and service names used in this website are for identification purposes only. Use of these names, trademarks and brands does not imply endorsement.