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) $\rightleftharpoons$ 2 HI(g)
When equilibrium is reached, the concentration of H₂(g) has decreased to 0.036 mol/L. What is the equilibrium constant, K_c, for the reaction?

Question

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)

\rightleftharpoons

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

Quizplus · Accepted Answer

The Answer of 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) $\rightleftharpoons$ 2 HI(g) When equilibrium is reached, the concentration of H₂(g) has decreased to 0.036 mol/L. What is the equilibrium constant, K_c, for the reaction?

At a High Temperature, Equal Concentrations of 0 ⇌\rightleftharpoons⇌ 2 HI(g) When Equilibrium Is Reached, the Concentration of H2(g)

At a High Temperature, Equal Concentrations of 0 $\rightleftharpoons$ 2 HI(g)
When Equilibrium Is Reached, the Concentration of H₂(g)