Consider the following equilibrium:
CO₂(g) + H₂(g) $\rightleftharpoons$ CO(g) + H₂O(g) ; K_c = 1.6 at 1260 K
Suppose 0.019 mol CO₂ and 0.030 mol H₂ are placed in a 3.00-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L · atm/K·mol)

Question

Consider the following equilibrium:
CO₂(g) + H₂(g)

\rightleftharpoons

CO(g) + H₂O(g) ; K_c = 1.6 at 1260 K
Suppose 0.019 mol CO₂ and 0.030 mol H₂ are placed in a 3.00-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L · atm/K·mol)

Quizplus · Accepted Answer

The Answer of Consider the following equilibrium: CO₂(g) + H₂(g) $\rightleftharpoons$ CO(g) + H₂O(g); K_c = 1.6 at 1260 K Suppose 0.019 mol CO₂ and 0.030 mol H₂ are placed in a 3.00-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/K·mol)

Consider the Following Equilibrium: CO2(g) + H2(g) ⇌\rightleftharpoons⇌ CO(g) + H2O(g); Kc = 1

Consider the Following Equilibrium:
CO₂(g) + H₂(g) $\rightleftharpoons$ CO(g) + H₂O(g); K_c = 1