For the reaction CO(g) + H₂O(g) CO₂(g) + H₂(g)
K = 3.88 at a certain temperature. If at this temperature in a certain experiment the equilibrium concentrations are [H₂] = 1.5 M, [CO₂] = 1.8 M, and [H₂O] = 0.26 M, calculate [CO].

Question

For the reaction CO(g) + H₂O(g) For the reaction CO(g) + H2O(g) CO2(g) + H2(g) K = 3.88 at a certain temperature. If at this temperature in a certain experiment the equilibrium concentrations are [H2] = 1.5 M, [CO2] = 1.8 M, and [H2O] = 0.26 M, calculate [CO]. A) 0.37 M B) 1.5 M C) 4.7 M D) 2.7 M E) none of these

For the reaction CO(g) + H<sub>2</sub>O(g) CO<sub>2</sub>(g) + H<sub>2</sub>(g) K = 3.88 at a certain temperature. If at this temperature in a certain experiment the equilibrium concentrations are [H<sub>2</sub>] = 1.5 M, [CO<sub>2</sub>] = 1.8 M, and [H<sub>2</sub>O] = 0.26 M, calculate [CO]. A) 0.37 M B) 1.5 M C) 4.7 M D) 2.7 M E) none of these

CO₂(g) + H₂(g)
K = 3.88 at a certain temperature. If at this temperature in a certain experiment the equilibrium concentrations are [H₂] = 1.5 M, [CO₂] = 1.8 M, and [H₂O] = 0.26 M, calculate [CO].

Quizplus · Accepted Answer

The equilibrium constant K is given by: K = [CO₂][H₂]/[H₂O][CO] Plugging in the given values, we get: 3.88 = (1.8)(1.5)/(0.26)[CO] Solving for [CO], we get: [CO] = (1.8)(1.5)/(0.26)(3.88) = 2.7 M Therefore, the answer is choice D, 2.7 M.

For the Reaction CO(g) + H2O(g) CO2(g) + H2(g)

For the Reaction CO(g) + H₂O(g) CO₂(g) + H₂(g)