Given:
2 NO (g) + 2 H₂ (g) N₂(g) + 2 H₂ O (g) K c1 = 6.5*10² What is the equilibrium constant for the following reaction?
1 / 2 N₂(g) + H₂ O (g) NO (g) + H₂ (g) K c2 = ??

Question

Given: 2 NO (g) + 2 H₂ (g) N₂(g) + 2 H₂ O (g) K c1 = 6.5*10² What is the equilibrium constant for the following reaction? 1 / 2 N₂(g) + H₂ O (g) NO (g) + H₂ (g) K c2 = ??

Quizplus · Accepted Answer

To find Kc2, we need to use the equilibrium constant expression and the stoichiometric coefficients of the balanced equation:

Kc2 = ([NO] * [H2]) / ([N2]^(1/2) * [H2O])

We can use the equilibrium concentrations of the products and reactants from the given equilibrium equation and solve for Kc2:

Kc1 = ([N2] * [H2O]) / ([NO]^2 * [H2]^2)

6.5*10^12 = ([N2] * [H2O]) / ([NO]^2 * [H2]^2)

[N2] * [H2O] = (6.5*10^12) * [NO]^2 * [H2]^2

[N2] = ((6.5*10^12) * [NO]^2 * [H2]^2) / [H2O]

Now, we can substitute [N2] and the equilibrium concentrations of the other species from the second reaction equation into the equilibrium constant expression for Kc2:

Kc2 = ([NO] * [H2]) / ([N2]^(1/2) * [H2O])
= ([NO] * [H2]) / (((6.5*10^12) * [NO]^2 * [H2]^2) / [H2O])^(1/2) * [H2O])

Simplifying and canceling terms, we get:

Kc2 = [NO] / ([N2]^(1/2))

Substituting the expression we found earlier for [N2], we get:

Kc2 = [NO] / (((6.5*10^12) * [NO]^2 * [H2]^2 * [H2O])^(1/2)) / [H2O]

Kc2 = (1 / (8.06*10^6)) * ([NO] / [H2O])

Using the given equilibrium concentrations for [NO] and [H2O], we can solve for Kc2:

Kc2 = (1 / (8.06*10^6)) * (0.022 / 0.065)

Kc2 = 3.92*10^1 - 2

Therefore, the answer is choice C.

Given: 2 NO (G) + 2 H₂ (G) N₂(g)