Chapter 13.3, Problem 23PP

(a)

Interpretation Introduction

Interpretation: The equilibrium expression for the following reaction should be determined:

  ${\text{2O}}_{\text{3}}\text{(g)}\rightleftarrows {\text{3O}}_{\text{2}}\text{(g)}$

Concept Introduction:

The relationship between the concentration of products and reactants at equilibrium for a general reaction:

  $\text{aA}\text{+}\text{bB}\rightleftarrows \text{cC}\text{+}\text{dD}$

Where A, B, C, and D represents chemical species and a, b, c, and d are the coefficients for balanced reaction.

The equilibrium expression, K_c for reversible reaction is determined by multiplying the concentrations of products together and divided by the concentrations of the reactants. Each concentration is raised to the power that is equal to the coefficient in the balanced reaction. So, the expression is:

  ${\text{K}}_{\text{c}}\text{=}\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$

Square brackets represent the concentration.

(b)

Interpretation Introduction

Interpretation: The equilibrium expression for the following reaction should be determined:

  ${\text{2NaHCO}}_{\text{3}}\text{(s)}\rightleftarrows {\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(s)}\text{+}{\text{CO}}_{\text{2}}\text{(g)}\text{+}{\text{H}}_{\text{2}}\text{O(g)}$

Concept Introduction:

The relationship between the concentration of products and reactants at equilibrium for a general reaction:

  $\text{aA}\text{+}\text{bB}\rightleftarrows \text{cC}\text{+}\text{dD}$

Where A, B, C, and D represents chemical species and a, b, c, and d are the coefficients for balanced reaction.

The equilibrium expression, K_c for reversible reaction is determined by multiplying the concentrations of products together and divided by the concentrations of the reactants. Each concentration is raised to the power that is equal to the coefficient in the balanced reaction. So, the expression is:

  ${\text{K}}_{\text{c}}\text{=}\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$

Square brackets represent the concentration.

(c)

Interpretation Introduction

Interpretation: The equilibrium expression for the following reaction should be determined:

  ${\text{C}}_{\text{6}}{\text{H}}_{\text{6}}\text{(g)}\text{+}{\text{3H}}_{\text{2}}\text{(g)}\rightleftarrows {\text{C}}_{\text{6}}{\text{H}}_{\text{12}}\text{(g)}$

Concept Introduction:

The relationship between the concentration of products and reactants at equilibrium for a general reaction:

  $\text{aA}\text{+}\text{bB}\rightleftarrows \text{cC}\text{+}\text{dD}$

Where A, B, C, and D represents chemical species and a, b, c, and d are the coefficients for balanced reaction.

The equilibrium expression, K_c for reversible reaction is determined by multiplying the concentrations of products together and divided by the concentrations of the reactants. Each concentration is raised to the power that is equal to the coefficient in the balanced reaction. So, the expression is:

  ${\text{K}}_{\text{c}}\text{=}\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$

Square brackets represent the concentration.

(d)

Interpretation Introduction

Interpretation: The equilibrium expression for the following reaction should be determined:

  $\text{4HCl(g)}\text{+}\text{Si(s)}\rightleftarrows {\text{SiCl}}_{\text{4}}\text{(l)}\text{+}{\text{2H}}_{\text{2}}\text{(g)}$

Concept Introduction:

The relationship between the concentration of products and reactants at equilibrium for a general reaction:

  $\text{aA}\text{+}\text{bB}\rightleftarrows \text{cC}\text{+}\text{dD}$

Where A, B, C, and D represents chemical species and a, b, c, and d are the coefficients for balanced reaction.

The equilibrium expression, K_c for reversible reaction is determined by multiplying the concentrations of products together and divided by the concentrations of the reactants. Each concentration is raised to the power that is equal to the coefficient in the balanced reaction. So, the expression is:

  ${\text{K}}_{\text{c}}\text{=}\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$

Square brackets represent the concentration.