# Problem: Consider the following system at equilibrium. 2CO(g)+O2(g) ↔ 2CO2(g)1. How will increasing the concentration of CO shift the equilibrium?A) to the rightB) to the leftC) no effect2. How will increasing the concentration of CO2 shift the equilibrium?A) to the rightB) to the leftC) no effect3. How will decreasing the volume of the container shift the equilibrium?A) to the rightB) to the leftC) no effect

###### FREE Expert Solution

We’re being asked to identify the effect of the changes for the given reaction:

2 CO(g)+O2(g) ↔ 2 CO2(g)

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.

1. How will increasing the concentration of CO shift the equilibrium?

• CO → reactant
• Adding reactant will favor the forward direction.

The equilibrium shifts A) to the right

2. How will increasing the concentration of CO2 shift the equilibrium?

•  CO2 → product
• Adding product will favor the reverse direction.

The equilibrium shifts B) to the left

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###### Problem Details

Consider the following system at equilibrium.

2CO(g)+O2(g) ↔ 2CO2(g)

1. How will increasing the concentration of CO shift the equilibrium?

A) to the right

B) to the left

C) no effect

2. How will increasing the concentration of CO2 shift the equilibrium?

A) to the right

B) to the left

C) no effect

3. How will decreasing the volume of the container shift the equilibrium?

A) to the right

B) to the left

C) no effect

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