Carbon monoxide (CO) reacts with hydrogen (H2) to form methane (CH4) and water (H20).
CO(g) + 3H2(g) + CH4(g)+H20(9)
The reaction is at equilibrium at 1,000 K. The equilibrium constant of the reaction is 3.90. At equilibrium, the concentrations are as
follows.
[CO] = 0.30 M
[H2] = 0.10 M
[H20] = 0.020 M
What is the equilibrium concentration of CH, expressed in scientific notation?
0.0059
5.9 x 10-2
0.059
5.9 x 102

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

The given balanced equilibrium reaction is,

[tex]CO(g)+3H_2(g)\rightleftharpoons CH_4(g)+H_2O(g)[/tex]

At eqm. conc. (0.30) M (0.10) M (x) M (0.020) M

The expression for equilibrium constant for this reaction will be,

[tex]K_c=\frac{[CH_4]\times [H_2O]}{[CO]\times [H_2]^3}[/tex]

Now put all the given values in this expression, we get :

[tex]3.90=\frac{x\times (0.020)}{(0.30)\times (0.10)^3}[/tex]

By solving the term 'x', we get :

x = 0.059 M= [tex]5.9\times 10^{-2}M[/tex]

Thus, the concentrations of [tex]CH_4[/tex] at equilibrium is :

Concentration of [tex]CH_4[/tex] = (x) M = [tex]5.9\times 10^{-2}M[/tex]

The equilibrium concentration of [tex]CH_4[/tex] , expressed in scientific notation is [tex]5.9\times 10^{-2}M[/tex]