Consider the reaction 3X + Y ⇔ 2W + Z.
At equilibrium, [X] is 7.0 M, [Y] is 6.0 M, [W] is 5.0 M and [Z] is 7.0 M at 298 K. The value of the equilibrium constant at this temperature is:
a) 0.085
b) 0.560
c) 1.800
d) 11.760
Write the Keq expression, substitute the values given and solve for Keq. Post your work if you have questions.
To find the value of the equilibrium constant (K) at a given temperature, we need to use the concentrations of the reactants and products at equilibrium. In this case, we are given the equilibrium concentrations of [X], [Y], [W], and [Z].
The equilibrium constant expression for this reaction is:
K = ([W]^2 * [Z]) / ([X]^3 * [Y])
Now we substitute the given equilibrium concentrations into the expression:
K = ([5.0 M]^2 * [7.0 M]) / ([7.0 M]^3 * [6.0 M])
Calculating:
K = (25 * 7) / (343 * 6)
K = 175 / 2058
K ≈ 0.085
Therefore, the value of the equilibrium constant at this temperature is approximately 0.085.
So the correct answer is (a) 0.085.