Consider the following equilibrium:
CO₂(g) + H₂(g)
CO(g) + H₂O(g) ; K_c = 1.6 at 1260 K
Suppose 0.037 mol CO₂ and 0.020 mol H₂ are placed in a 3.50-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)

Consider the following equilibrium: CO<sub>2</sub>(g) + H<sub>2</sub>(g) CO(g) + H<sub>2</sub>O(g) ; K<sub>c</sub> = 1.6 at 1260 K Suppose 0.037 mol CO<sub>2</sub> and 0.020 mol H<sub>2</sub> are placed in a 3.50-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L ∙ atm/(K ∙ mol) ) A) 4.1 atm B) 0.5 atm C) 1.6 atm D) 1.1 atm E) 0.59 atm

CO(g) + H₂O(g) ; K_c = 1.6 at 1260 K
Suppose 0.037 mol CO₂ and 0.020 mol H₂ are placed in a 3.50-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) CO(g)+ H₂O(g); K_c = 1.6 at 1260 K Suppose 0.037 mol CO₂ and 0.020 mol H₂ are placed in a 3.50-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