# Question #bc2ab

##### 1 Answer

#### Explanation:

The idea here is that keeping the *temperature* and the *number of moles of gas* **constant** will allow you to use Boyle's Law to calculate how the volume of the gas will change following that increase in pressure.

As you know, Boyle's Law states that when temperature and number of moles of gas are kept **constant**, pressure and volume have an **inverse relationship**.

Simply put, when pressure *increases*, volume **decreases**, and when pressure *decreases*, volume **increases**.

Mathematically, Boyle's Law can be written like this

#color(blue)(P_1V_1 = P_2V_2)" "# , where

Plug your values and solve this equation for **do not** forget to convert the final pressure from *mmHg* to *atm* by using the conversion factor

#"1 atm " = " 760 mmHg"#

#P_1V_1 = P_2V_2 implies V_2 = P_1/P_2 * V_1#

#V_2 = (1.50color(red)(cancel(color(black)("atm"))))/(1240/760color(red)(cancel(color(black)("atm")))) * "5.0 L" = color(green)("4.6 L")#

Notice how the volume *decreased* as a result of the *increase* in pressure.