Calculate the value of the equilibrium constant for the following reaction based on the given concentrations of reactants and products. N2 = 1.5 M, H2 = 0.5 M, NH3 = 2 M
N2 (g) + H2 (g) ↔ NH3 (g)
Are those the equilibrium concentrations? I assume they are. Writ the Keq expression, substitute those numbers and solve for Keq. Post your work if you get stuck.
To calculate the value of the equilibrium constant (K) for the given reaction, you need to use the concentrations of the reactants and products at equilibrium. The equilibrium constant, also known as the law of mass action, relates these concentrations.
In this case, the balanced equation is:
N2 (g) + 3H2 (g) ↔ 2NH3 (g)
The equilibrium constant expression is given by:
K = [NH3]² / ([N2] * [H2]³)
Now, plug in the given concentrations into the expression:
[N2] = 1.5 M
[H2] = 0.5 M
[NH3] = 2 M
K = (2 M)² / ((1.5 M) * (0.5 M)³)
Simplifying the equation:
K = 4 M² / (1.5 M * 0.5 M³)
K = 4 / (1.5 * 0.5³)
K = 4 / (1.5 * 0.125)
K = 4 / 0.1875
K = 21.33