The equilibrium constant, Kc, for the reaction H2 (g) + I2 (g) ⇄ 2HI (g) at 425°C is 54.8. A reaction vessel contains 0.0890 M HI, 0.215 M H2, and 0.498 M I2. Which statement is correct about this reaction mixture?
a. The reaction quotient is greater than 1.
b. The reaction is not at equilibrium and will proceed to make more products to reach equilibrium.
c. The reaction mixture is at equilibrium.
d. The reaction is not at equilibrium and will proceed to make more reactants to reach equilibrium.

b. The reaction is not at equilibrium and will proceed to make more products to reach equilibrium.

Explanation:

Step 1: Data given

Kc at 425 °C = 54.8

[HI] = 0.498 M

[H2] = 0.215 M

[I2] = 0.498 M

Step 2: The balanced equation

H2 (g) + I2 (g) ⇄ 2HI (g)

Step 3: Calculate Q

Kc = 54.8

Q = [HI]² / [H2][I2]

Q = (0.0890)² / (0.215)(0.498) = 0.074

When Q<<Kc, there are more reactants than products. As a result, some of the reactants will become products, causing the reaction to shift to the right

Option B is correct: b. The reaction is not at equilibrium and will proceed to make more products to reach equilibrium.

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.

ill try to . no promises tho.

explanation: