An equilibrium mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 3.77 10-3 mol/L, [O2] = 4.30 10-3 mol/L, and [SO3] = 4.13 10-3 mol/L. Calculate the equilibrium constant, K, for the following reaction.
2 SO2(g) + O2(g) 2 SO3(g)
Write the equilibrium constant expression, substitute the numbers in the problem and solve for Kc.
i did that, but it was wrong, can you show me the correct formula to use
nevermind, i got the correct answer of 279
To calculate the equilibrium constant, K, for the given reaction, you need to use the concentrations of the reactants and products at equilibrium.
The equilibrium constant expression for the reaction is:
K = [SO3]^2 / ([SO2]^2 * [O2])
Given the concentrations at equilibrium:
[SO2] = 3.77 * 10^-3 mol/L
[O2] = 4.30 * 10^-3 mol/L
[SO3] = 4.13 * 10^-3 mol/L
Plugging in the values into the equilibrium constant expression:
K = (4.13 * 10^-3 mol/L)^2 / ((3.77 * 10^-3 mol/L)^2 * (4.30 * 10^-3 mol/L))
K = (0.0170 mol^2/L^2) / (0.0126 * 10^-3 mol^2/L^2)
K = (0.0170 mol^2/L^2) / (0.0126 * 10^-3 mol^2/L^2)
K = 1.35 * 10^3
Therefore, the equilibrium constant, K, for the given reaction is 1.35 * 10^3.