Chapter 15, Problem 15.58SP

Interpretation Introduction

(a)

Interpretation:

The equilibrium constant expression for K_p and the equation that relates K_p and K_c for the equation ${\text{CH}}_4(g){\text{ + H}}_2\text{O(g) }\rightleftharpoons {\text{ CO(g) + 3 H}}_2\text{(g)}$ should be given.

Concept introduction:

Equilibrium constant expression for gas-phase reactions are written using partial pressures.

$\text{aA(g) }\rightleftharpoons \text{ bB(g) + cC(g)}$

${\text{K}}_P=\frac{{\left(P_B\right)}^b{\left(P_C\right)}^c}{{\left(P_A\right)}^a}$

P_A, P_B and P_C are partial pressures of A, B and C gases respectively.

The concentration or partial pressure of pure solids and pure liquids are not included in the equilibrium constant expression.

The relationship between K_p and K_c is given by the following equation.

$K_p=K_c{\left(RT\right)}^{\Delta n}$

K_p = equilibrium constant in terms of partial pressure

K_c = equilibrium constant in terms of concentrations.

R = universal gas constant

T = absolute temperature

$\Delta n=\text{ moles of gaseous products - moles of gaseous reactants}$

Interpretation Introduction

(b)

Interpretation:

The equilibrium constant expression for K_p and the equation that relates K_p and K_c for the equation $3{\text{ F}}_2{\text{(g) + Cl}}_2\text{(g) }\rightleftharpoons {\text{ 2 ClF}}_3\text{(g)}$ should be given.

Concept introduction:

Equilibrium constant expression for gas-phase reactions are written using partial pressures.

$\text{aA(g) }\rightleftharpoons \text{ bB(g) + cC(g)}$

${\text{K}}_P=\frac{{\left(P_B\right)}^b{\left(P_C\right)}^c}{{\left(P_A\right)}^a}$

P_A, P_B and P_C are partial pressures of A, B and C gases respectively.

The concentration or partial pressure of pure solids and pure liquids are not included in the equilibrium constant expression.

The relationship between K_p and K_c is given by the following equation.

$K_p=K_c{\left(RT\right)}^{\Delta n}$

K_p = equilibrium constant in terms of partial pressure

K_c = equilibrium constant in terms of concentrations.

R = universal gas constant

T = absolute temperature

$\Delta n=\text{ moles of gaseous products - moles of gaseous reactants}$

Interpretation Introduction

(c)

Interpretation:

The equilibrium constant expression for K_p and the equation that relates K_p and K_c for the equation ${\text{H}}_2{\text{(g) + F}}_2\text{(g)}\rightleftharpoons \text{ 2 HF(g)}$ should be given.

Concept introduction:

Equilibrium constant expression for gas-phase reactions are written using partial pressures.

$\text{aA(g) }\rightleftharpoons \text{ bB(g) + cC(g)}$

${\text{K}}_P=\frac{{\left(P_B\right)}^b{\left(P_C\right)}^c}{{\left(P_A\right)}^a}$

P_A, P_B and P_C are partial pressures of A, B and C gases respectively.

The concentration or partial pressure of pure solids and pure liquids are not included in the equilibrium constant expression.

The relationship between K_p and K_c is given by the following equation.

$K_p=K_c{\left(RT\right)}^{\Delta n}$

K_p = equilibrium constant in terms of partial pressure

K_c = equilibrium constant in terms of concentrations.

R = universal gas constant

T = absolute temperature

$\Delta n=\text{ moles of gaseous products - moles of gaseous reactants}$