# You transfer a sample of gas at 17°C from a volume of 4.81 L and 1.10 atm to a container at 37°C that has a pressure of 1.10 atm. What is the new volume of the gas?

##### 1 Answer

#### Explanation:

An important thing to notice here is that, unless the question is mistyped, the **pressure** of the gas is being kept **constant**.

If you take into account the fact that the *number of moles* of gas is constant as well, you can say that the *change in volume* will only depend on the *change in temperature*.

As you know, when number of moles of gas and pressure are kept constant, volume and temperature have a **direct relationship** - this is known as Charles' Law.

So, when temperature **Increases**, the volume **increases** as well. Likewise, when temperature **decreases**, the volume **decreases** as well.

In your case, the temperature increased from *increase*.

Mathematically, Charles' Law is expressed as

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

Rearrange to solve for **no not** forget that the temperature of the gas **must** be expressed in *Kelvin*!

#V_2 = T_2/T_1 * V_1#

In your case, this will be equal to

#V_2 = ( (273.15 + 17) color(red)(cancel(color(black)("K"))))/( (273.15 + 37) color(red)(cancel(color(black)("K")))) * "4.81 L"#

#V_2 = "6.641 L"#

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

#V_2 = color(green)("6.6 L")#

**SIDE NOTE** *If the pressure of the gas is not constant, you can solve the problem by using the combined gas law equation*

#color(blue)((P_1V_1)/T_1 = (P_2V_2)/T_2)" "# , where

*the pressure, volume, and temperature of the gas at an initial state*

*the pressure, volume, and temperature of the gas at a final state*