Respuesta :
The given question is incomplete. The complete question is :
Calculate to three significant digits the density of boron trifluoride gas at exactly −5°C and exactly 1 atm . You can assume boron trifluoride gas behaves as an ideal gas under these conditions.
Answer: The density of boron trifluoride gas is 3.08 g/L
Explanation:
To calculate the relation of density and molar mass of a compound, we use the ideal gas equation:
PV=nRT
P = pressure = 1 atm
V = Volume
n = number of moles
R = gas constant =0.0821 Latm/Kmol
T = temperature = [tex]-5^0C=(273-5)= 268K[/tex]
Number of moles (n) can be written as:
[tex]n=\frac{m}{M}[/tex]
where, m = given mass
M = molar mass
[tex]PV=\frac{m}{M}RT\\\\PM=\frac{m}{V}RT[/tex]
where,
[tex]\frac{m}{V}=d[/tex]
where d = density
The relation becomes:
PM=dRT
[tex]d=\frac{PM}{RT}[/tex]
[tex]d=\frac{1atm\times 67.82g/mol}{0.0821Latm/Kmol\times 268K}=3.08g/L[/tex]
Thus the density of boron trifluoride gas is 3.08 g/L
