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

To the right.

Explanation:

The chemical equilibrium is a state of a reactant system in which they are not observed changes as time goes by, even though the reaction continues. In other words, the chemical equilibrium is established when there are two opposite reactions which take place simultaneously at the same speed.

The variation in the concentration of any of the species involved in the equilibrium varies the value of the concentrations of the remaining species in the equilibrium.

In this case the concentration of one of the reaction reagents varies, increasing it since there is a greater amount of CO. This causes the balance to change to the products to compensate for the reaction. Then the balance goes to the right.

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

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.