) Consider the reaction: N2(g) + O2(g) ⇌ 2 NO(g). If [N2] = 0.520 M, [O2] = 0.0662 M, and [NO] = 0.00956 at equilibrium, calculate the value of K and describe the physical/chemical interpretation
To calculate the value of K, we use the formula for the equilibrium constant:
K = [NO]^2 / ([N2] * [O2])
Plugging in the given values:
K = (0.00956)^2 / (0.520 * 0.0662)
K = 0.0000910736 / 0.034392
K = 0.002648
Therefore, the value of K for the reaction N2(g) + O2(g) ⇌ 2 NO(g) is 0.002648.
Interpretation:
The equilibrium constant K tells us the ratio of products to reactants at equilibrium. In this case, the value of K = 0.002648 indicates that at equilibrium, the concentrations of NO are dominant compared to N2 and O2. This suggests that the forward reaction (N2(g) + O2(g) -> 2 NO(g)) is favored at equilibrium, resulting in the production of more NO gas molecules from N2 and O2.