Question

A sample of gas has a mass of 827 mg . Its volume is 0.270 L at a temperature of 88 ∘ C and a pressure of 975 mmHg . Find its molar mass.

Answer 1

Steps:

Mw = w * R * T / p * V

T = 88 + 273 => 361 K

p = 975 mmHg in atm :

1 atm = 760 mmHg

975 mmg / 760 mmHg => 1.28 atm

Therefore:

= 0.827 * 0.0821 * 361 / 1.28 * 0.270

= 24.51 / 0.3456

molar mass = 70.92 g/mol

Answer 2

The molar mass of the gas is 70.83 g/mol.

Step-by-step explanation:

Mass of the gas m= 827 mg = 0.827 g

Molar mass of gas = M

Pressure of the gas = 975 mmHg = 1.28 atm

Temperature of the gas = 88^C= 361 K

Using idal gas equation:

`PV=nRT`

`PV=(m)/(M)* RT`

`M=(mRT)/(PV)`

`M=(0.827 g* 0.0820 atm L/mol K* 361 K)/(1.28 atm * 0.270 L)=70.83 g/mol`

The molar mass of the gas is 70.83 g/mol.