Answer:
K = 9.4 *10^5
The reaction favor product formation
Explanation:
Equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium. Also it is defined as the ratio of the product of concentration of products to the product of concentration of reactants each term raised to power equal their stochiometric coefficients.
so, for the reaction,
- 2H₂ ₍g₎ + S₂ ₍g₎ → 2H₂S ₍g₎
The equilibrium constant can be expressed as following:
where concentration of reactants and products is expressed in molarity Molarity=(no of moles/ Volume L)
So,
[H₂] = (0.50 mol / 1 L) = 0.50 M
[S₂] = (0.02 mol / 1 L) = 0.020 M
[H₂S] = (68.5 mol / 1 L) = 68.5 M
∴ K_{eq}=\frac{[68.5]^2}{0.50]^2\times [0.020]}=9.4*10^5
As the value of K is greater than 1, the reaction favor product formation.