Question

The equilibrium constant, Keq, is 4. 4 × 10-4 at 500 K. 2 Upper N Upper O Upper C l (g) double-headed arrow 2 Upper N Upper O (g) Upper C l Subscript 2 Baseline (g) Determine the direction of reaction if 1. 00 M NOCl is combined with 0. 500 M NO and 0. 500 M Cl2 in a sealed flask. No reaction occurs. Reaction proceeds to the right toward the products. Reaction proceeds to the left toward the reactants. Reaction proceeds to the left toward the products.

Answer 1

The reaction at the given concentration proceed towards left to form reactants. Thus, option C is correct.

The given balanced equation has been:

$\rm 2\;NOCl\;\leftrightharpoons 2\;NO\;+\;Cl_2$

The equilibrium constant, Keq for the reaction, is given as:

$Keq=\rm \dfrac{[NO]^2\;[Cl_2]}{[NOCl]^2}$

Computation for direction of reaction

The given concentration of NOCl is 1 M

The given concentration of NO is  0. 5 M

The given concentration of Chlorine is  0. 5 M.

The value of equilibrium constant for given concentrations are:

$Keq=\dfrac{[ 0. 5]^2\;[ 0. 5]}{[1]^2}\\ Keq=0.125$

The given value of equilibrium constant is $\rm 4.4\;\times\;10^-^4$. Since the given value of constant is less than the reaction constant, the reaction proceeds towards the reactant  to establish equilibrium.

Thus, option C is correct.

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