# Problem: Consider the following reaction at equilibrium:2 CO2(g) ⇌ 2 CO(g) + O2(g)                ∆H° = –514 kJThe prediction is that adding O2(g) to the reaction container will lead to a(n):A. increase in the partial pressure of CO(g)B. decrease in the partial pressure of CO2(g)C. increase in the value of the equilibrium constantD. increase in the partial pressure of CO2(g)E. decrease in the value of the equilibrium constant

###### FREE Expert Solution

We are asked to predict what happens when we add O2(g) to the reaction.

2 CO2(g) ⇌ 2 CO(g) + O2(g)                ∆H° = –514 kJ

According to Le Chatelier’s Principle, if a system (chemical reaction) is at equilibrium and we disturb it, then the system will readjust to maintain its equilibrium state.

When we add reactants or remove products the chemical reaction will shift in the forward direction to re-establish equilibrium. This causes an increase in the products and a decrease in the reactants. Products and Reactants (Forward Direction)

When we remove reactants or add products the chemical reaction will shift in the reverse direction to re-establish equilibrium. This causes a decrease in the products and an increase in the reactants. Products and Reactants (Reverse Direction)

94% (268 ratings) ###### Problem Details

Consider the following reaction at equilibrium:

2 CO2(g) ⇌ 2 CO(g) + O2(g)                ∆H° = –514 kJ

The prediction is that adding O2(g) to the reaction container will lead to a(n):

A. increase in the partial pressure of CO(g)

B. decrease in the partial pressure of CO2(g)

C. increase in the value of the equilibrium constant

D. increase in the partial pressure of CO2(g)

E. decrease in the value of the equilibrium constant