Chemical Equilibrium

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This is a 8 point assignment

Objectives: After completing this unit, students should be able to:

1. Given the balanced equation of a reversible chemical reaction, write the equilibrium constant expression.
2. Given the equilibrium constant for one reaction, determine the value of the equilibrium constant for a related reaction.
3. Relate equilibrium constant magnitude to the position of the equilibrium and the relative equilibrium concentrations of reactants and products.
4. Write an equilibrium expression for reactions involving a solid or a liquid.
5. Given the concentrations of all reacting species, calculate the reaction quotient, Q and predict the direction of reaction.
6. Calculate K_p or K_c from each of the following:
   1. Equilibrium concentrations or partial pressures of all species.
   2. Initial concentrations and one equilibrium concentration.
7. Use the equilibrium constant to calculate equilibrium concentrations.
8. 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:

Introduction

13.1 Chemical Equilibria

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:

13.2 Equilibrium Constants

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:

13.2 Equilibrium Constants

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:

13.2 Equilibrium Constants

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:

13.2 Equilibrium Constants

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:

13.2 Equilibrium Constants

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:

13.4 Equilibrium Calculations

Question 18:

Question 19:

Question 20:

Question 21: