# If 12 L of a gas at room temperature exerts a pressure of 64 kPa on its container, what pressure will the gas exert if the container's volume changes to 24 L?

Jul 10, 2016

The container now has a pressure of 32kPa.

#### Explanation:

Let's start off with identifying our known and unknown variables.

The first volume we have is $12$ L, the first pressure is $64 k P a$, and the second volume is $24 L$. Our only unknown is the second pressure.

We can obtain the answer using Boyle's Law which shows that there is an inverse relationship between pressure and volume as long as the temperature and number of moles remain constant.

The equation we use is:

All we have to do is rearrange the equation to solve for ${P}_{2}$

We do this by dividing both sides by ${V}_{2}$ in order to get ${P}_{2}$ by itself:
${P}_{2} = \frac{{P}_{1} \times {V}_{1}}{V} _ 2$

Now all we have to do is plug in the given values:
${P}_{2} = \left(64 \setminus k P a \times 12 \setminus \cancel{\text{L")/(24\cancel"L}}\right)$ = $32 k P a$