Question

The density of a gas is 1.43 g/l at a temperature of 23 ∘c and a pressure of 0.789 atm. Calculate the molar mass of the gas.

Answer 1

Answer: 44.04 g/mol

Step-by-step explanation:

Ideal gas law in terms of density:

`PV=nRT\\\\PV=(w)/(M)* RT\\\\M=(w)/(V)* (RT)/(P)\\\\M=\rho* (RT)/(P)`

where,

P = pressure of the gas = 0.789 atm

V = volume of the gas

T = temperature of the gas =
`23^0C=(23+273)=296K`

n = number of moles of the gas

R = gas constant = 0.0821 Latm/moleK

M = molar mass of gas

w = mass of gas

`\rho` = density =1.43 g/ml

`M=1.43* (0.0821* 296)/(0.789)`

`M=44.04g/mol`

Thus molar mass of the gas is 44.04 g/mol