Chapter 7, Problem 66P

(a)

Interpretation Introduction

Interpretation:Whether the given reaction is at equilibrium or not needs to be identified.

Concept Introduction:

For any equilibrium reaction, the equilibrium constant expression can be represented as follows:

$K=\frac{\left[\text{Product}\right]}{\left[\text{Reactant}\right]}$

(b)

Interpretation Introduction

Interpretation:The direction in which the reaction proceed to reach equilibrium needs to be determined.

Concept Introduction:

For any equilibrium reaction, the equilibrium constant expression can be represented as follows:

$K=\frac{\left[\text{Product}\right]}{\left[\text{Reactant}\right]}$

The direction of reaction to reach equilibrium will depends on its Q or quotient reaction value. If the value of Q is greater than K thus, reaction moves in backward direction to form more reactant and if the value of Q is less than K thus, reaction moves in forward direction to form more product.

(c)

Interpretation Introduction

Interpretation:If the reactants remain at the same equilibrium concentrations, the concentration of product in order to establish equilibrium needs to be determined.

Concept Introduction:

For any equilibrium reaction, the equilibrium constant expression can be represented as follows:

$K_{eq}=\frac{\left[\text{Product}\right]}{\left[\text{Reactant}\right]}$

Here, $\left[\text{Product}\right]$ is equilibrium concentration of product and $\left[\text{Reactant}\right]$ is equilibrium concentration of reactant.