The question is incomplete, here is the complete question:
A sample of gas weighs 10.1 g and occupies a volume of 5.65 L at 60 °C and 580 torr. Identify the gas sample.
(a) [tex]CHCl_3[/tex] (molar mass = 119.4 g/mol)
(b) [tex]N_2O[/tex] (molar mass = 44.02 g/mol)
(c) [tex]SO_2[/tex] (molar mass = 64.07 g/mol)
(d) [tex]NH_3[/tex] (molar mass = 17.03 g/mol)
(e) [tex]Cl_2[/tex] (molar mass = 70.90 g/mol)
Answer: The gas sample is [tex]SO_2[/tex] having molar mass of 64 g/mol
Explanation:
To calculate the molar mass of the gas, we use the equation given by ideal gas equation:
PV = nRT
Or,
[tex]PV=\frac{w}{M}RT[/tex]
where,
P = Pressure of the gas = 580 torr
V = Volume of the gas = 5.65 L
w = Weight of the gas = 10.1 g
M = Molar mass of gas = ?
R = Gas constant = [tex]62.36\text{ L. Torr }mol^{-1}K^{-1}[/tex]
T = Temperature of the gas = [tex]60^oC=[60+273]K=333K[/tex]
Putting values in above equation, we get:
[tex]580torr\times 5.65L=\frac{10.1g}{M}\times 62.364\text{ L. torr }mol^{-1}K^{-1}\times 333K\\\\M=\frac{10.1\times 62.364\times 333}{580\times 5.65}=64g/mol[/tex]
Hence, the gas sample is [tex]SO_2[/tex] having molar mass of 64 g/mol
