These laws describe the relationships between the physical quantities **pressure**, **volume** and **temperature** as they relate to gases.

## Why Learn the Gas Laws?

- The gas laws tell us how gases behave when subjected to various
*pressures*($P$), made to fit into certain*volumes*($V$) or kept at specific*absolute temperatures*($T$) - Very important when combinations of these situations are considered
- Each law usually keeps one physical quantity constant while varying the others so as to have us see the relationship between those varied quantities

### Boyle’s Law

- Named after physicist and chemist Robert Boyle
- The
**pressure***of a fixed mass of gas***is inversely proportional to**its**volume***at a constant temperature*:

Thus we can have $P_1V_1=k$ and $P_2V_2=k$. Combining these two we get: $$ \begin{equation}\begin{aligned} P_1V_1=P_2V_2\\ \end{aligned}\end{equation} $$ Where $P_1$ is the pressure associated with the gas of volume $V_1$ and $P_2$ is associated with $V_2$.

##### Example

A small balloon is filled with $0.005\ m^3$ of air and has a pressure of $108\ kPa$.

If the balloon is squeezed to cause it to have a lower volume of $0.004\ m^3$, determine the new pressure inside of the balloon.

If the balloon can only withstand a pressure of $111\ kPa$, does the balloon pop in the process of squeezing it to this new volume?

#### Mission details

A gas exerts a pressure of $3\ kPa$ on the walls of container 1. When container 1 is emptied into a $10\ m^3$ container, the pressure exerted by the gas increases to $6\ kPa$. Find the volume of container 1.