# Question #c83bc

##### 1 Answer

#### Explanation:

Since it's obvious that the question was mistyped, I will use the values given to you to show how volume **decreases** as a result of an **increase** in pressure.

You don't need to convert *torr* to *atm* because both the initial and the final pressure are expressed in *atm*.

The problem doesn't mention the *temperature* and *number of moles* of gas, which means that you can assume that they are being **kept constant**, When that is the case, pressure and volume have an **inverse relationship** described by **Boyle's Law**.

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

In your case, pressure **increases** from **decreases**.

Mathematically, Boyle's Law can be expressed as

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

Rearrange to solve for

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

Plug in your values to get

#V_2 = (2.5 color(red)(cancel(color(black)("atm"))))/(4.50color(red)(cancel(color(black)("atm")))) * "2 L" = color(green)(|bar(ul(color(white)(a/a)"1.1 L"color(white)(a/a)|)))#

I'll leave the answer rounded to two **sig figs**, despite the fact that you only have one sig fig for the initial volume of the gas.

As predicted, the volume **decreased** as a result of the *increase* in pressure.