# Question #68dd9

##### 1 Answer

#### Explanation:

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

When this is the case, *pressure* and *volume* have an **inverse relationship** - this is known as **Boyle's Law**.

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

This means that right from the start, you can look at the fact that the volume of the gas *decreases* and say that the pressure **must** *increase*.

Mathematically, this is expressed as

#color(blue)(|bar(ul(color(white)(a/a)P_1V_1 = P_2V_2color(white)(a/a)|)))" "# , where

Rearrange to solve for the pressure of the gas at the final state,

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

Plug in your values to get

#P_2 = (6.00 color(red)(cancel(color(black)("L"))))/(1.40color(red)(cancel(color(black)("L")))) * "760 torr" = "3257.1 torr"#

Rounded to two **sig figs**, the number of sig figs you have for the initial pressure of the gas, the answer will be

#P_2 = color(green)(|bar(ul(color(white)(a/a)"3300 torr"color(white)(a/a)|)))#