# If 18 L of a gas at room temperature exerts a pressure of 35 kPa on its container, what pressure will the gas exert if the container's volume changes to 14 L?

Jun 9, 2016

The new pressure is $45 k P a$

#### Explanation:

Let's start off with identifying our known and unknown variables.
The first volume we have is $18$ L, the first pressure $35 k P a$ and the second volume is $14 L$. 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 ${P}_{1} {V}_{1} = {P}_{2} {V}_{2}$
where the numbers 1 and 2 represent the first and second conditions. All we have to do is rearrange the equation to solve for the pressure.

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

Now all we do is plug and chug!
${P}_{2} = \left(35 \setminus k P a \times 18 \setminus \cancel{\text{L")/(14\cancel"L}}\right)$ = $45$ $k P a$