Answer: 44.04 g/mol
Explanation:
Ideal gas law in terms of density:
[tex]PV=nRT\\\\PV=\frac{w}{M}\times RT\\\\M=\frac{w}{V}\times \frac{RT}{P}\\\\M=\rho\times \frac{RT}{P}[/tex]
where,
P = pressure of the gas = 0.789 atm
V = volume of the gas
T = temperature of the gas = [tex]23^0C=(23+273)=296K[/tex]
n = number of moles of the gas
R = gas constant = 0.0821 Latm/moleK
M = molar mass of gas
w = mass of gas
[tex]\rho[/tex] = density =1.43 g/ml
[tex]M=1.43\times \frac{0.0821\times 296}{0.789}[/tex]
[tex]M=44.04g/mol[/tex]
Thus molar mass of the gas is 44.04 g/mol
