Question

Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH₄(????) + H₂O(????) ⇌ 3H₂(????) + CO(????) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH₄, 0.126 M; H₂O, 0.242 M; CO, 0.126 M; H₂ 1.15 M, at a temperature of 760 °C?

Answer 1

6.2846

Step-by-step explanation:

Given that:-

Concentrations at equilibrium :-

`[CH_4]=0.126\ M`

`[H_2O]= 0.242\ M`

`[CO]= 0.126\ M`

`[H_2]= 1.15\ M`

The equilibrium reaction is:-

`CH_4+H_2O\rightleftharpoons 3H_2+CO`

The expression for equilibrium constant is:

`K_(c)=\frac {\left [ H_2 \right ]^3\left [ CO \right ]}{\left [ CH_4 \right ]\left [ H_2O \right ]}`

Applying the values as:-

`K_c=(1.15^3* 0.126)/(0.126* 0.242)=6.2846`

The equilibrium constant for the reaction is:- 6.2846