At a certain temperature the reaction CO₂(g) + H₂(g) CO(g) + H₂O(g)
Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

Question

At a certain temperature the reaction CO₂(g) + H₂(g)

At a certain temperature the reaction CO<sub>2</sub>(g) + H<sub>2</sub>(g) CO(g) + H<sub>2</sub>O(g) Has K<sub>c</sub> = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide? A) 0.091 M B) 0.191 M C) 0.209 M D) 0.913 M E) 1.05 M

CO(g) + H₂O(g)
Has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

Quizplus · Accepted Answer

According to the balanced chemical equation, the stoichiometry of the reaction is 1:1 for both CO₂ and H₂. Therefore, at equilibrium, the concentrations of CO and H₂O will also be 1:1. Let x be the equilibrium concentration of CO (in mol/L). Then, at equilibrium, the concentrations of CO₂ and H₂ will be (2.00 - x) and (1.5 - x), respectively. Using the expression for the equilibrium constant and plugging in the equilibrium concentrations, we get: K_c = [CO][H₂O]/[CO₂][H₂] 2.50 = x(x)/(2.00 - x)(1.5 - x) Solving for x, we get x = 0.209 M. Therefore, the concentration of CO at equilibrium is 0.209 M, which corresponds to choice (C).

At a Certain Temperature the Reaction CO2(g) + H2(g)

At a Certain Temperature the Reaction CO₂(g) + H₂(g)