AP Chemistry Unit 7 Quiz - Equilibrium and Solubility Questions

Sep 29, 2026

AP Chemistry Unit 7 quiz focused on chemical equilibrium and solubility concepts. It tests equilibrium-constant expressions for Kc and Kp, identification of when equilibrium is reached from concentration-vs-time behavior, and how temperature, pressure, concentration, and added reactants/products affect Q versus K and shift outcomes. Additional questions evaluate Ksp relationships, solubility product reasoning for ionic compounds, and equilibrium behavior in dissolution reactions using given initial amounts and pressures.

LanguageEnglish

CategoryExam

FormatPDF

Pages8

Reading Time20 min

AccessFree to download

Equilibrium Constants and Expressions

Kc expressions for gas-phase reactions

Kp expressions and partial-pressure calculations

Equilibrium Shifts and Reaction Quotient

Pressure/temperature effects at constant temperature

Q vs K behavior when adding reactants

Solubility Product (Ksp) and Dissolution Equilibria

AgBr and AgI solubility/Ksp relationships

PbCl2 Ksp calculations

Overall Ksp/dissolution outcomes with initial conditions

AP Chemistry Unit 7 Quiz 1. N2(g)+3H2(g)⇋2NH3(g) Given the reaction above, what is the equilibrium constant, Kc? a. Kc= [N2][H2]3/[2NH3]2 b. Kc= [NH3]/[H2][N2] c. Kc= [NH3]2/[H2]3 [N2] d. Kc= [N2][H2]/[NH3] 2. The graph above presents the relationship of concentration of products and reactants asthe reaction progresses. Which point of time was equilibrium reached? a. 0 b. 0.75 c. 1 d. 1.5 3. At a constant temperature, which of the following reactions would be affected from a change in pressure? a. 2SO2(g)+O2(g)⇋2SO3(g) b. N2(g)+H2(g)⇋2NH3(g) c. 2HI(g)⇋H2(g)+I2(g) d. 2NO(g)⇋N2(g)+O2(g) 4. At a constant temperature, an increase in pressure would lead to an increase in product for which of the following reactions? a. 2NO(g)⇋N2(g)+O2(g) b. H2(g)+CO2(g)⇋H2O (g)+CO(g) c. CO(g)+Cl2(g)⇋COCl2(g) d. 2N2O 5(g)⇋4NO2(g)+O2(g) 5. CaCO3(g)+energy⇋CaO(s)+CO2(g) The given reaction above takes place in a container. Given the reaction, which of the following changes would lead to an increase in the concentration of CO2(g)? a. An increase in temperature b. A decrease in temperature c. An increase in container d. A decrease in container H2(g)+I2(g)⇋2HI △H =58kj/mol The reaction provided is in an equilibrium at 25°C. 6. What is the expression of the equilibrium constant for the reaction? a. Kc= [H2][I2]/[HI]2 b. Kc= [HI]2/[H2][I2] c. Kc= [HI]/[H2][I2] d. Kc= [H2][I2]/[HI] 7. Which of the following changes would affect the reverse reaction to speed up? a. Increase the temperature b. Decrease the temperature c. Increase the concentration of I2 d. Decrease the pressure 8. Which of the following would lead to a reduction in the value of the equilibrium constant? a. Decrease the temperature b. Increase the temperature c. Increase the concentration of I2 d. Decrease the pressure 9. The value of the Kc is 5.0. Which of the following would result in order to reach equilibrium if the initial concentration of all three species is 3.0? a. No change would occur. b. The rate of forward reaction will increase. c. The rate of reverse reaction will increase. d. Both sides of the reaction will increase. 10. 2NO(g)⇋N2(g)+O2(g) From the reaction given above, what is the expression of the equilibrium constant, Kp? a. Kp=(O2)(N2)/(NO)2 b. Kp=(O2)(N2)/(NO) c. Kp=(NO)2/(O2)(N2) d. Kp=(NO)/(O2)(N2) 11. The reaction provided above has reached equilibrium at a certain temperature. During that time, the partial pressure due to NO was 3 atmospheres, the partial pressure due to N2 was 2 atmospheres, and the partial pressure due to O2 was 3 atmospheres. What is the value of the equilibrium constant, Kp? a. 1/3 b. 2/3 c. 1 d. 2 12. The Ksp value of AgBr is 7.7*10-13. Which of the following is equal to the solubility of AgBr? a. 7. 7*10-13 molar b. 5.9*10-25 molar c. 8.8*10-7 molar d. 3. 7*10-13 molar 13. Pb2+(aq) + Zn(s)⇋Pb(s)+Zn2+(aq) Keq=3*1030. A student performed an experiment where he put a 0.20 mol sample of solid zinc into a 500mL solution of 1.0MPbSO3(aq). After a long period of time, what would be a possible result? a. Half of the concentration of Zn solid remains. b. One-third of the concentration of Zn solid remains. c. All of the concentration of Zn solid remains. d. None of the concentration of Zn solid remains. 14. The solubility of AgI is 8.0*10-17 . What is the solubility product constant, Ksp, for AgI? a. 1.6*10-16 b. 8.9*10-9 c. 8*10-17 d. 6.4*10-33 15. Which of the following expressions is equal to the Ksp of PbCl2 ? a. Ksp= [Pb2+][Cl-] b. Ksp= [Pb2+]2 [Cl-] c. Ksp= [Pb2+][Cl-]2 d. Ksp= [Pb2+]2 [Cl-]2 16. PbCl2(s)⇋Pb2+(aq)+2Cl-(aq). If [Pb2+]=3.2*10-10M at equilibrium at a certain temperature, which of the following provides the correct Ksp for PbCl2 ? a. 1.3*10-28 M b. 1.0*10-19 M c. 5. 1*10-20 M d. 8.2*10-30 M 17. N2(g) + O2(g) ⇋ 2NO(g) The given reaction initially contained 3 moles of N

FAQs

How do you write the Kc expression for a reaction like N2 + H2 ⇌ NH3?

Use the equilibrium concentrations of the species raised to their stoichiometric coefficients, with products in the numerator and reactants in the denominator.

How does increasing pressure at constant temperature affect product yield for a given equilibrium?

Pressure favors the side with fewer moles of gas. Choose the reaction where the product side has fewer gas moles than the reactant side.

What does a change in temperature do to the value of the equilibrium constant (K)?

Changing temperature changes K. For these questions, a decrease in temperature lowers K while an increase in temperature raises K, as specified by the intended equilibrium direction.

Sep 29, 2026

Upload by 8796093062539