Question

User Suppose that for the reaction 2N2O(g)+O2(g).....4NO(g) it is determined, at a particular temperature, that the equilibrium concentrations are [NO(g)] = 0.00294 M, [N2O(g)]= 0.0161 M, and [O2(g)] = 0.0350 M. Calculate the value of K for the reaction at this temperature. K=?

Answer 1

The equilibrium constant (K) for the reaction 2N2O(g) + O2(g) ⇌ 4NO(g), given the equilibrium concentrations, is calculated to be K = 8.10×10^-6.

Step-by-step explanation:

To calculate the equilibrium constant (K) for the given reaction 2N2O(g) + O2(g) ⇌ 4NO(g), we use the equilibrium concentrations of the products and reactants. The equilibrium expression for this reaction is K = [NO]4 / ([N2O]2 * [O2]). Substituting the given concentrations, we get K = (0.00294 M)4 / ((0.0161 M)2 * (0.0350 M)).

Calculating this value gives us:

K = ((0.00294)4) / ((0.0161)2 * 0.0350)
K = (7.4846×10-8) / (9.2321×10-3)
K = 8.10×10-6

Therefore, the equilibrium constant for the reaction at this temperature is K = 8.10×10-6.