Home > Class 11 Biology > 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. 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 __________.
2. 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 __________.
3. In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.
4. 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.
5. 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.
6. 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 __________.
7. 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.
8. 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 __________.
9. What role did Karl Bosch play in development of the Haber-Bosch process?
10. 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, __________.
11. 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)
12. 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 __________.
13. The effect of a catalyst on a chemical reaction is to react with product, effectively removing it and shifting the equilibrium to the right.
14. Kp = 0.0198 at 721 K for the reaction 2HI (g) H2 (g) + I2 (g)
In a particular experiment, the partial pressures of H2 and I2 at equilibrium are 0.710 and 0.888 atm, respectively. The partial pressure of HI is __________ atm.
15. Which one of the following is true concerning the Haber process?
16. 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.
17. 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.
18. 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 __________.
19. 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 __________.
20. 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).
21. 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 __________.
22. 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 __________.
23. 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?
24. 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)
25. 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 __________.

⚡ Recently practiced quizzes in this topic
Live quiz activity
Class 11 Biology: Cell - The Unit of Life Class 11 Biology Practice Test: The Living World - Diversity in the Living World Class 11 Biology Practice Test: Structural Organisations in Animals - Frogs Class 11 Biology Practice Test: Morphology of Flowering Plants - Flower Class 11 Biology Practice Test: Morphology of Flowering Plants - Fabaceae, Solanaceae and Lillaceae Class 11 Biology: Animal Kingdom Class 11 Biology Practice Test: Cell The Unit of Life - Prokaryotic Cells Class 11 Biology Practice Test: Cell The Unit of Life - Nucleus Class 11 Biology: Plant Kingdom Class 11 Biology Practice Test: Plant Growth and Development - Differentiation, Dedifferentiation & Redifferentiation
 
❤ 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 | 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.