# For the reaction, "CaCO"_3"(s)" ⇌ "CaO(s) + CO"_2"(g)",what will happen in each of the followig cases?

## (a) you add some carbon dioxide (b) you lower the pressure (c) you remove some calcium oxide (d) you increase the volume

Feb 20, 2017

Here's what I get.

#### Explanation:

This is an exercise on Le Châtelier's Principle, which states that

When a stress is applied to a system at equilibrium, the system will respond in such a way as to relieve the stress.

The system at equilibrium is

$\text{CaCO"_3"(s)" ⇋ "CaO(s)" + "CO"_2"(g)}$

Adding ${\text{CO}}_{2}$

The system will respond to remove ${\text{CO}}_{2}$.

The position of equilibrium will move to the left and the mass of ${\text{CaCO}}_{3}$ will increase.

Lowering the pressure

The system will try to increase the pressure by producing more ${\text{CO}}_{2}$.

The position of equilibrium will move to the right and the mass of ${\text{CaCO}}_{3}$ will decrease.

Removing some $\text{CaO}$

Changing the amount of a solid has no effect on the position of equilibrium.

The mass of ${\text{CaCO}}_{3}$ will be unchanged.

Increasing the volume

Increasing the volume will decrease the pressure of ${\text{CO}}_{2}$.

The system will try to increase the pressure by producing more ${\text{CO}}_{2}$.

The position of equilibrium will move to the right and the mass of ${\text{CaCO}}_{3}$ will decrease.