Question

The gaseous product of a reaction is collected in a 25.0L container at 27.0 C. The pressure in the container is 3.0atm and the gas has a mass of 96.0g. What is the molar mass of the gas?

Answer 1

Answer: The molar mass of the gas is 31.6 g/mol

Step-by-step explanation:

According to ideal gas equation:

`PV=nRT`

P = pressure of gas = 3.0 atm

V = Volume of gas = 25.0 L

n = number of moles = ?

R = gas constant =
`0.0821Latm/Kmol`

T =temperature =
`27.0^0C=(27.0+273)K=300K`

`n=(PV)/(RT)`

`n=(3.0atm* 25.0L)/(0.0821 L atm/K mol* 300K)=3.04moles`

Moles =
`\frac{\text {given mass}}{\text {Molar mass}}`

`3.04=\frac{96.0g}{\text {Molar mass}}`

`{\text {Molar mass}}=31.6g/mol`

The molar mass of the gas is 31.6 g/mol