Question

Consider the following reaction: CO(g)+2H2(g) <--> CH3OH(g).

An equilibrium mixture of this reaction at a certain temperature was found to have
[CO]=0.115M, [H2]=0.116M, and [CH3OH]=0.190M. What is the value of the equilibrium constant (Kc) at this temperature?

Answer 1

123 is the equilibrium constant for the reaction.

Step-by-step explanation:

`CO(g)+2H_2(g)\rightleftharpoons CH_3OH(g)`

Equilibrium concentration of reactants :

`[CO]=0.115 M,[H_2]=0.116 M`

Equilibrium concentration of products:

`[CH_3OH]=0.190 M`

The expression of an equilibrium constant is given by :

`K_c=([CH_3OH])/([CO][H_2]^2)`

`K_c=(0.190 M)/(0.115 M* (0.116 M)^2)`

`K_c=122.78 \approx 123`

123 is the equilibrium constant for the reaction.