The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N₂O₄(g) ⇌ 2NO₂(g) K = 1.46
3N₂O₄(g) ⇌ 6NO₂(g) K = ?

Question

The equilibrium constant is given for one of two reactions below. Determine the value of the missing equilibrium constant. N₂O₄(g) ⇌ 2NO₂(g) K = 1.46 3N₂O₄(g) ⇌ 6NO₂(g) K = ?

Quizplus · Accepted Answer

For the second reaction, the equilibrium constant can be determined using the following equation:

K = ([NOS]^6) / ([NSO2]^3 * [O2])

We can use the equilibrium constant from the first reaction to solve for [NSO2]:

K = ([NOS]^2) / [NSO2]

[NSO2] = ([NOS]^2) / K

Substituting this expression into the equation for K in the second reaction gives:

K = ([NOS]^6) / ([([NOS]^2) / K]^3 * [O2])

Simplifying:

K = K * [NOS]^6 / ([NOS]^6 * [O2])

K = 1 / [O2]

Therefore, the missing equilibrium constant is K = 1 / 1.46 = 0.685. The best choice is C.

The Equilibrium Constant Is Given for One of Two Reactions