Consider the following equilibrium:
CO₂(g) + H₂(g) CO(g) + H₂O(g) ; K_c = 1.6 at 1260 K
Suppose 0.038 mol CO₂ and 0.022 mol H₂are placed in a 1.50-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 0.038 mol CO<sub>2</sub> and 0.022 mol H<sub>2 </sub>are placed in a 1.50-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L · atm/K·mol) A) 9.9 atm B) 1.1 atm C) 4.1 atm D) 2.6 atm E) 1.5 atm

CO(g) + H₂O(g) ; K_c = 1.6 at 1260 K
Suppose 0.038 mol CO₂ and 0.022 mol H₂are placed in a 1.50-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 0.038 mol CO₂ and 0.022 mol H₂are placed in a 1.50-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