If 0.520 mol nitrogen has a volume of 17.0 L at some temperature and pressure, what volume would 0.750 mol carbon dioxide have at the same temperature and pressure?

24.52 mL

Explanation:

Data obtained from the question include:

Number of mole of N2 = 0.52 mole

Volume of N2 = 17L

Number of mole of CO2 = 0.750 mol

Next, we need to obtain the volume of 0.750 mole N2.

This is illustrated below:

Initial volume (V1) = 17L

Initial mole (n1) = 0.52 mole

Final volume (V2) =.?

Final mole (n2) = 0.750 mole

PV = nRT

Divide both side by n

PV/n = RT

Divide both side by P

V/n = RT/P

Since pressure (P) and temperature (T) are constant, then

V/n = constant

V1/n1 = V2/n2

With the above equation, we can obtain the new volume of N2 as follow:

V1/n1 = V2/n2

17/0.52 = V2/0.75

Cross multiply to express in linear form

0.52 x V2 = 17 x 0.75

Divide both side by 0.52

V2 = (17 x 0.75) /0.52

V2 = 24.52 mL.

The volume occupied by 0.75 mole of N2 is 24.52 mL.

Since 0.750 mole of CO2 is under the same temperature and pressure as 0.750 mole of N2, they will both occupy the same volume.

Therefore, 0.750 mole of CO2 will occupy 24.52 mL

the dependant variable is spilled water

the independent is the heat