Question

If you have 0.56 moles of an ideal gas at 87 ° C and a pressure of 569 torr, what volume will the gas take up?

Answer 1

The ideal gas law: PV = nRT

Conversions: 
87°C = 360K
P = 0.75 atm
R = 0.0821
n = 0.56

0.75V = (0.56)(0.0821)(360)

V = 22 L

Answer 2

Explanation:

The given data is as follows.

            n = 0.56 moles,              T = $87^{o}C$ = (87 + 273) K = 360 K

            P = 569 torr = 0.748 atm (as 1 torr = 0.0013 atm)

According to ideal gas equation, PV = nRT

Therefore, putting given values into the above formula as follows.

                           PV = nRT

     $0.748 \times V = 0.56 \times 0.0821 L atm/mol K \times 360 K$

                     V = 22.12 L

Thus, we can conclude that the given gas will take up 22.12 L of volume.