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.

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.

At a high temperature,equal concentrations of 0.160 mol/L of H<sub>2</sub>(g) and I<sub>2</sub>(g) are initially present in a flask.The H<sub>2</sub> and I<sub>2</sub> react according to the balanced equation below. When equilibrium is reached,the concentration of H<sub>2</sub>(g) has decreased to 0.036 mol/L.What is the equilibrium constant,K<sub>c</sub>,for the reaction? A) 3.4 B) 4.0 C) 12 D) 22 E) 48

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

First, we need to use the given concentrations to calculate the initial moles of each reactant: mol(H₂) = 0.160 mol/L x V (volume of the solution) mol(I₂) = 0.160 mol/L x V (volume of the solution) At equilibrium, we know that the concentration of H₂(g) is 0.036 mol/L, so we can use the equation to calculate the concentration of I₂(g): K_c = ([I₂]^11/[H₂]^11) 0.036^11 / (0.124)^11 = 48.4 K_c ≈ 48 (rounded to the nearest whole number) Therefore, the best choice is E) 48.

At a High Temperature,equal Concentrations of 0