Answer: The molar mass of the given unknown compound is 50.5 g/mol.
Explanation:
To calculate the volume of water, we use the equation given by ideal gas, which is:
[tex]PV=nRT[/tex]
or,
[tex]PV=\frac{m}{M}RT[/tex]
where,
P = pressure of sample = 1.00 atm
V = volume of sample = 2010 mL = 2.010 L (Conversion factor: 1 L = 1000 mL)
m = Given mass of unknown compound = 2.73 g
M = Molar mass of unknown compound = ? g/mol
R = Gas constant = [tex]0.0820\text{ L atm }mol^{-1}K^{-1}[/tex]
T = temperature of sample = [tex]180^oC=[180+273]K=453K[/tex]
Putting values in above equation, we get:
[tex]1.00atm\times 2.010L=\frac{2.73g}{M}\times 0.0820\text{ L atm }mol^{-1}K^{-1}\times 453K\\\\V=50.45g/mol[/tex]
Rounding off to 3 significant figures, we get the molar mass to be 50.5 g/mol.
Hence, the molar mass of the given unknown compound is 50.5 g/mol.
