# Question #d8985

##### 1 Answer

#### Explanation:

Before doing ny calculations, try to predict what's going to happen to the volume of the gas.

You know that when pressure and number of moles are kept **constant**, volume and temperature have a **direct relationship**.

Simply put, **increasing** the temperatue will lead to an *increase* in volume, and **decreasing** the temperature will lead to a *decrease* in volume - this is known as Charles' Law.

So, why would that be the case?

Remember that gas pressure is caused by molecules bumpoing into the walls of the container. *Temperature* as we know it is simply a measure of the **average kinetic energy** of the molecules that make up the gas sample.

So, *higher temperature* means that the molecules are moving faster, and thus hitting the walls of the container *more often* and with *more force* **increases**.

Mathematically, Charles' Law is written like this

#color(blue)(V_1/T_1 = V_2/T_2)" "# , where

**A very important** thing to remember here is that temperature **must be** expressed in Kelvin!

So, plug in your values and solve for

#V_2 = T_2/T_1 * V_1#

#V_2 = ((273.15 + 100.0)color(red)(cancel(color(black)("K"))))/((273.15 + 20.0)color(red)(cancel(color(black)("K")))) * "3.50 L" = "4.4551 L"#

Rounded to three sig figs, the answer will be

#V_2 = color(green)("4.46 L")#

Indeed, an increase in temperature lead to an increase in volume!