Given: C(s)+ CO₂(g) 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g)and CO₂(g)are 1.22 atm and 0.780 atm,respectively.Calculate the value of K for this reaction.

Question

Quizplus · Accepted Answer

The equilibrium constant (Kp) for the given reaction can be calculated using the expression:

Kp = (P(CO))^2 / P(COS)

Where P(CO) and P(COS) are the partial pressures of CO and COS at equilibrium, respectively.

Substituting the given values, we get:

Kp = (1.22 atm)^2 / 0.780 atm = 1.91

Therefore, the best choice is C) 1.91.

Given: C(s)+ CO2(g) 2CO(g) at Equilibrium at a Certain

Given: C(s)+ CO₂(g) 2CO(g) at Equilibrium at a Certain