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sergeinik [125]
3 years ago
10

Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH₄(????) + H₂O(????) ⇌ 3

H₂(????) + 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?
Chemistry
1 answer:
sammy [17]3 years ago
5 0

Answer:

6.2846

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=\frac{1.15^3\times 0.126}{0.126\times 0.242}=6.2846

<u>The equilibrium constant for the reaction is:- 6.2846</u>

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