Chapter 14, Problem 14.21P

Interpretation Introduction

Interpretation:

Using the initial partial pressures of ${\text{H}}_{\text{2}}\text{O}$ , $\text{CO}$ , and ${\text{H}}_{\text{2}}$ we can find their equilibrium partial pressures at 1000 K for the reaction $C_{(g)}+H_2{O}_{(g)}\rightleftharpoons C{O}_{(g)}+H_2{}_{(g)}$ .

Concept introduction:

Partial Pressure is defined as the pressure an individual gas exerts. It is independent of other gases that may be present in a mixture.  According to the ideal gas law, partial pressure is inversely proportional to volume. It is also directly proportional to moles and temperature.

Given:

The initial partial pressures of P_CO=1.00 atm and P_H2=1.40 atm.

The equilibrium constant K_p for the reaction is $C_{(g)}+H_2{O}_{(g)}\rightleftharpoons C{O}_{(g)}+H_2{}_{(g)}$ 2.44 at 1000 K.

To determine:

The equilibrium partial pressures of ${\text{H}}_{\text{2}}\text{O}$ , $\text{CO}$ , and ${\text{H}}_{\text{2}}$ at 1000 K for the reaction $C_{(g)}+H_2{O}_{(g)}\rightleftharpoons C{O}_{(g)}+H_2{}_{(g)}$