# Problem: At a high temperature, equal concentrations of 0.160 mol/L of H2(g) and I2(g) are initially present in a flask. The H2 and I2 react according to the balanced equation below. H2(g) + I2(g) ⇌ 2 HI(g)When equilibrium is reached, the concentration of H2(g) has decreased to 0.036 mol/L. What is the equilibrium constant, Kc, for the reaction?a. 0.00522b. 33c. 6.89d. 9.68e. 47

###### FREE Expert Solution

We are being asked to calculate the equilibrium constant, Kc for the given equilibrium reaction:

H2(g) + I2(g) ⇌ 2 HI(g)

When dealing with equilibrium and Kc:

Kc → equilibrium units are in molarity
Kc is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only aqueous and gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the concentrations in the equilibrium expression

Given:

###### Problem Details

At a high temperature, equal concentrations of 0.160 mol/L of H2(g) and I2(g) are initially present in a flask. The H2 and I2 react according to the balanced equation below.

H2(g) + I2(g) ⇌ 2 HI(g)

When equilibrium is reached, the concentration of H2(g) has decreased to 0.036 mol/L. What is the equilibrium constant, Kc, for the reaction?

a. 0.00522
b. 33
c. 6.89
d. 9.68
e. 47