# Question #34022

##### 1 Answer

#### Answer:

Here's how you can solve this problem.

#### Explanation:

Notice that the problem doesn't mention *temperature* and *number of moles of gas*, which means that you can assume that they are **constant**.

This implies that you can use the equation for **Boyle's Law** to find the volume of the gas at a pressure of

#color(blue)(ul(color(black)(P_1V_1 = P_2V_2)))#

Here

#P_1# and#V_1# are the pressure and volume of the gas at an initial state#P_2# and#V_2# are the pressure and volume of the gas at a final state

What you have to do here is to rearrange the above equation to solve for

#P_1 * V_1 = P_2 * V_2 implies V_2 = P_1/P_2 * V_1#

At this point, you would plug in your values and find the value of *milliliters* and must have three **sig figs**.

So, to sum this up, Boyle's Law tells you that when temperature and number of moles of gas are kept **constant**, the pressure and the volume of the gas have an **inverse relationship**.

This means that when pressure **increases**, the volume of the gas must **decrease** by the factor. Similarly, when pressure **increases**, the volume of the gas must **increase** by the same factor.

In your case, the pressure **decreases** from **increase**.

#P_2 < P_1 implies V_2 > V_1#