Question

I, 0.215 M H2, and 0.498 M I2. Which statement is correct about this reaction mixture? View Available Hint(s) 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? The reaction is not at equilibrium and will proceed to make more reactants to reach equilibrium. The reaction quotient is greater than 1. The reaction is not at equilibrium and will proceed to make more products to reach equilibrium. The reaction mixture is at equilibrium.

Answer 1

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

Explanation:  

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as $K_{eq}$

K is the constant of a certain reaction when it is in equilibrium, while Q is the reaction  quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

$H_2(g)+I_2(g)\rightarrow 2HI(g)$

The expression for $Q$ is written as:

$Q=\frac{[HI]^2}{[H_2]^1[I_2]^1}$

$Q=\frac{[0.0890]^2}{[0.215]^1[0.498]^1}$

$Q=0.074$

Given : $K_{eq}$ = 54.8

Thus as $Q$, the reaction will shift towards the right i.e. towards the product side.