This is a 8 point assignment
Objectives: After completing this unit, students should be able to:
- Given the balanced equation of a reversible chemical reaction, write the equilibrium constant expression.
- Given the equilibrium constant for one reaction, determine the value of the equilibrium constant for a related reaction.
- Relate equilibrium constant magnitude to the position of the equilibrium and the relative equilibrium concentrations of reactants and products.
- Write an equilibrium expression for reactions involving a solid or a liquid.
- Given the concentrations of all reacting species, calculate the reaction quotient, Q and predict the direction of reaction.
- Calculate Kp or Kc from each of the following:
- Equilibrium concentrations or partial pressures of all species.
- Initial concentrations and one equilibrium concentration.
- Use the equilibrium constant to calculate equilibrium concentrations.
- Based on Le Chatelier’s principle explain how relative equilibrium quantities of reactants and products are shifted by changes to the equilibrium conditions.
Reading and Homework Exercises
Table of Contents from: OpenStax Chemistry 2e: Chapter 13
Question 1 addresses your general understanding of chemical equilibrium.
You might find the following reading in OpenStax helpful:
Question 1:
Objective 1 and 4 Practice – Questions 2-6 test your ability identify correct expressions for the equilibrium constant (K).
You might find the following reading in OpenStax helpful:
Question 2:
Question 3:
Question 4:
Question 5:
Question 6:
Objective 6 part 1 Practice – Questions 7 and 8 test your ability to calculate the value of the equilibrium constant (K) given equilibrium concentrations
You might find the following reading in OpenStax helpful:
Question 7:
Question 8:
Objective 5 Practice – Questions 9-13 test your understanding of the reaction quotient Q and its use
You might find the following reading in OpenStax helpful:
Question 9:
Question 10:
Question 11:
Question 12:
Question 13:
Objective 3 Practice – Questions 14 and 15 test your understanding of how the relative position of an equilibrium can be predicted knowing the magnitude of K
You might find the following reading in OpenStax helpful:
Question 14:
Question 15:
Objective 2 Practice – Question 16 test your understanding of the values of K for related reactions
You might find the following reading in OpenStax helpful:
Question 16:
Objective 8 Practice question 17 tests your understanding of LeChatlier’s principle
You might find the following reading in OpenStax helpful:
13.3 Shifting Equilibria: Le Châtelier’s Principle
Question 17: For the reaction:
Cu2+ (aq) + 2 NH2OH (aq) ↔ Cu (s) + N2 (g) + 2 H2O (l) + 2 H+ (aq)
The reaction is exothermic
Answer the questions by filling in the blanks
Question 17:
Objective 6 part 2 and Objective 7 Practice – Questions 18-21 test your understanding of equilibrium constant calculations
You might find the following reading in OpenStax helpful:
Question 18:
Question 19:
Question 20:
Question 21: