Consider the chemical reaction 2NH₃(g) ⇌ N₂(g) + 3H₂(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g) are present. Estimate the equilibrium concentration of H₂(g).

Question

Quizplus · Accepted Answer

We can set up an ICE (initial, change, equilibrium) table and use the equilibrium constant to solve for the equilibrium concentrations: 2NH₃(g) ⇌ N₂(g) + 3H₂(g) I 1.22 M 0 0 C -2x +x +3x E 1.22 - 2x x 3x Kc = [N₂][H₂]3/[NH₃]2 = 4.0 × 10^-10 Substituting in the equilibrium concentrations: 4.0 × 10^-10 = (x)(3x)^3/(1.22 - 2x)^2 Solving for x: x = 20 M Therefore, the equilibrium concentration of H₂(g) is 20 M, which corresponds to choice B.

Consider the Chemical Reaction 2NH3(g) ⇌ N2(g) + 3H2(g)

Consider the Chemical Reaction 2NH₃(g) ⇌ N₂(g) + 3H₂(g)