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Carbon monoxide (CO) reacts with hydrogen (H2) to form methane (CH4) and water (H2O). Upper C upper O (g) plus 3 upper H subscript 2 (g) double-headed arrow upper C upper H 4 (g) plus upper H subscript 2 upper O (g). 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 [H2O] = 0. 020 M What is the equilibrium concentration of CH4 expressed in scientific notation? 1959 5. 9 x 10-2 0. 059 5. 9 x 102.

Sagot :

The equilibrium constant has been the ratio of the product and the reactant concentration raised to the stoichiometric coefficient. The equilibrium concentration of methane is 0.059 M.

What is equilibrium?

The equilibrium can be defined as the condition in which the rate of formation of product and the rate of breakdown of product is equal.

The given reaction has been:

[tex]\rm CO+3\;H_2\;\leftrightharpoons\;CH_4+H_2O[/tex]

The equilibrium constant (kc) for the reaction has been given as :

[tex]k_c=\rm \dfrac{[CH_4][H_2O]}{[CO][H_2]^3}[/tex]

Substituting the values of the equilibrium concentration in the equation as:

[tex]k_c=\dfrac{[\text C\text H_4][0.020]}{[0.30][0.10]^3} \\\\3.90=\dfrac{[\text C\text H_4]\;\times\;0.020}{0.0003} \\\\\rm CH_4=0.059\;M[/tex]

The equilibrium concentration of methane is 0.059 M. Thus, option C is correct.

Learn more about equilibrium concentration, here:

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