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:

Kc=productsreactants

▪ 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:    

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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

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