Consider the reaction: 2 H2S(g)--><-- 2H2(g) + S2 Kp= 2.4 x 10^-4 at 1073k

A reaction mixture contains .112 atm of H2,.055 atm of S2, and .445 atm of H2S. Is the reaction mixture at equlibrium? If not, in what direction will the reaction proceed?

To determine if the reaction mixture is at equilibrium, we need to compare the given pressures of the gases to the equilibrium constant, Kp.

The equilibrium constant (Kp) is calculated using the partial pressures of the species involved in the reaction. For the given reaction: 2 H2S(g) ⇌ 2H2(g) + S2, the expression for Kp is:

Kp = [H2]^2 [S2] / [H2S]^2

Let's substitute the given pressures into the equation and see if the calculated value of Kp matches the given value of 2.4 x 10^-4:

[Kp] = [(0.112 atm)^2 * (0.055 atm)] / [(0.445 atm)^2]

[Kp] ≈ 0.0011904

The calculated value of Kp is approximately 0.0011904, which is not equal to the given value of 2.4 x 10^-4. Therefore, the reaction mixture is not at equilibrium.

To determine the direction in which the reaction will proceed, we compare the calculated value of Kp to the given value:

1. If Kp > 2.4 x 10^-4, the reaction will proceed in the reverse direction to reach equilibrium.
2. If Kp < 2.4 x 10^-4, the reaction will proceed in the forward direction to reach equilibrium.

In this case, 0.0011904 > 2.4 x 10^-4, so the reaction will proceed in the reverse direction to reach equilibrium.

To determine if the reaction mixture is at equilibrium, we need to compare the calculated value of Kp with the given Kp value.

Step 1: Write the balanced equation for the reaction:
2 H2S(g) ⇌ 2H2(g) + S2(g)

Step 2: Calculate the reaction quotient Qp:
Qp = (P(H2))^(2) * P(S2) / (P(H2S))^2

Given pressures:
P(H2) = 0.112 atm
P(S2) = 0.055 atm
P(H2S) = 0.445 atm

Substituting the values into Qp:
Qp = (0.112)^2 * 0.055 / (0.445)^2

Qp ≈ 0.000331 (using a calculator)

Step 3: Compare Qp with Kp:
Qp = 0.000331
Kp = 2.4 × 10^(-4)

Since Qp > Kp, the reaction has not reached equilibrium.

Step 4: Determine the direction in which the reaction will proceed:
Since Qp is greater than Kp, the reaction will shift in the reverse direction to reach equilibrium. This means that more reactants (H2 and S2) will be produced, and the concentration of H2S will decrease until Qp equals Kp.