Example 14.1 Expressing Equilibrium Constants for Chemical Equations For Practice 14.1 Express the equilibrium constant for the combustion of propane as shown by the balanced chemical equation:
Example 14.2 Manipulating the Equilibrium Constant to Reflect Changes in the Chemical Equation For Practice 14.2 Consider the following chemical equation and equilibrium constant at 25 C: Calculate the equilibrium constant for the following reaction at 25 C: For More Practice 14.2 Predict the equilibrium constant for the first reaction shown here given the equilibrium constants for the second and third reactions:
Example 14.3 Relating K p and K c For Practice 14.3 Consider the following reaction and corresponding value of K c : What is the value of K p at this temperature?
Example 14.4 Writing Equilibrium Expressions for Reactions Involving a Solid or a Liquid For Practice 14.4 Write an equilibrium expression (K c ) for the equation:
Example 14.5 Finding Equilibrium Constants from Experimental Concentration Measurements For Practice 14.5 The reaction in Example 14.5 between CO and H 2 is carried out at a different temperature with initial concentrations of [CO] = 0.27 M and [H 2 ] = 0.49 M. At equilibrium, the concentration of CH 3 OH is 0.11 M. Find the equilibrium constant at this temperature.
Example 14.6 Finding Equilibrium Constants from Experimental Concentration Measurements For Practice 14.6 The reaction of CH 4 in Example 14.6 is carried out at a different temperature with an initial concentration of [CH 4 ] = 0.087 M. At equilibrium, the concentration of H 2 is 0.012 M. Find the equilibrium constant at this temperature.
Example 14.7 Predicting the Direction of a Reaction by Comparing Q and K For Practice 14.7 Consider the reaction and its equilibrium constant: A reaction mixture contains [NO 2 ] = 0.0255 M and [N 2 O 4 ] = 0.0331 M. Calculate Q c and determine the direction in which the reaction will proceed.
Example 14.8 Finding Equilibrium Concentrations When You Know the Equilibrium Constant and All but One of the Equilibrium Concentrations of the Reactants and Products For Practice 14.8 Diatomic iodine [I 2 ] decomposes at high temperature to form I atoms according to the reaction: In an equilibrium mixture, the concentration of I 2 is 0.10 M. What is the equilibrium concentration of I?
Example 14.9 Finding Equilibrium Concentrations from Initial Concentrations and the Equilibrium Constant For Practice 14.9 The reaction in Example 14.9 is carried out at a different temperature at which K c = 0.055. This time, however, the reaction mixture starts with only the product, [NO] = 0.0100 M, and no reactants. Find the equilibrium concentrations of N 2, O 2, and NO at equilibrium.
Example 14.10 Finding Equilibrium Concentrations from Initial Concentrations and the Equilibrium Constant For Practice 14.10 The reaction in Example 14.10 is carried out at the same temperature, but this time the reaction mixture initially contains only the reactant, [N 2 O 4 ] = 0.0250 M, and no NO 2. Find the equilibrium concentrations of N 2 O 4 and NO 2.
Example 14.11 Finding Equilibrium Partial Pressures When You Are Given the Equilibrium Constant and Initial Partial Pressures For Practice 14.11 The reaction between I 2 and Cl 2 in Example 14.11 is carried out at the same temperature, but with these initial partial pressures: = 0.150 atm, = 0.150 atm, P ICl = 0.00 atm. Find the equilibrium partial pressures of all three substances.
Example 14.12 Finding Equilibrium Concentrations from Initial Concentrations in Cases with a Small Equilibrium Constant For Practice 14.12 The reaction in Example 14.12 is carried out at the same temperature with the following initial concentrations: [H 2 S] = 0.100 M, [H 2 ] = 0.100 M, and [S 2 ] = 0.00 M. Find the equilibrium concentration of [S 2 ].
Example 14.13 Finding Equilibrium Concentrations from Initial Concentrations in Cases with a Small Equilibrium Constant Continued For Practice 14.13 The reaction in Example 14.13 is carried out at the same temperature with the following initial concentrations: [H 2 S] = 1.00 10 4 M, [H 2 ] = 0.00 M, and [S 2 ] = 0.00 M. Find the equilibrium concentration of [S 2 ].
Example 14.14 The Effect of a Concentration Change on Equilibrium For Practice 14.14 Consider the following reaction in chemical equilibrium: What is the effect of adding additional Br 2 to the reaction mixture? What is the effect of adding additional BrNO?
Example 14.15 The Effect of a Volume Change on Equilibrium For Practice 14.15 Consider the following reaction at chemical equilibrium: What is the effect of decreasing the volume of the reaction mixture? Increasing the volume of the reaction mixture?
Example 14.16 The Effect of a Temperature Change on Equilibrium For Practice 14.16 The following reaction is exothermic: What is the effect of increasing the temperature of the reaction mixture? Decreasing the temperature?