Consider the reaction:
2H2S(g)⇌2H2(g)+S2(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [H2S]= 0.542M , [H2]= 2.64×10−2M , and [S2]= 7.54×10−3M .
What is the value of the equilibrium constant at this temperature?
To find the value of the equilibrium constant (K) at a given temperature, you need to use the equation relating the concentrations of the reactants and products to K. In this case, the equation is:
K = ([H2]^2 * [S2]) / [H2S]^2
Now, let's substitute the given concentrations into the equation:
[H2S] = 0.542 M
[H2] = 2.64×10^−2 M
[S2] = 7.54×10^−3 M
K = ((2.64×10^−2)^2 * (7.54×10^−3)) / (0.542^2)
K = (7.00×10^−5 * 5.70×10^−5) / 0.293924
K = 3.99×10^−9
Therefore, the value of the equilibrium constant (K) at this temperature is 3.99×10^−9.
To calculate the equilibrium constant (K) for the given reaction, we need to use the concentrations of the reactants and products at equilibrium.
Using the equation for the equilibrium constant (K):
K = ([H2]^2 × [S2]) / [H2S]^2
Substituting the given concentrations:
K = ((2.64×10−2)^2 × (7.54×10−3)) / (0.542)^2
Simplifying the expression:
K = (0.0699 × 7.54×10−3) / (0.542)^2
K = 5.283×10^-6 / 0.294964
K ≈ 1.794×10^-5