Question

Consider the following system at equilibrium.2CO(g) + O2(g)<----> 2 CO2 (g)How will increasing the concentration of CO shift the equilibrium?a.to to the rightb.to the leftc.no effect

Answer 1

Adding more CO to the equilibrium reaction 2CO(g) + O2(g) ↔ 2CO2(g) will shift the equilibrium to the right, favoring the production of CO2.

Step-by-step explanation:

Increasing the concentration of CO in the equilibrium reaction 2CO(g) + O2(g) ↔ 2CO2(g) will shift the equilibrium to the right. This is in accordance with Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. In this case, by adding more CO, the system will try to reduce the increased concentration of CO by producing more CO2, thus shifting the equilibrium towards the products.

Answer 2

The position of equilibrium moves to the right (to CO2)

Step-by-step explanation:

Step 1: Data given

Step 2: The balanced equation

2CO(g) + O2(g) → 2CO2 (g)

Step 3:

Changing the concentration will shift the equilibrium to the side that would reduce that change in concentration.

According to Le Chatelier, the position of equilibrium will move in such a way as to counteract the change.

That means that the position of equilibrium will move so that the concentration of CO decreases again - by reacting it with O2 and turning it into CO2.

The position of equilibrium moves to the right.