Question

Calculate to three significant digits the density of boron trifluoride gas at exactly and exactly . You can assume boron trifluoride gas behaves as an ideal gas under these conditions.

Answer 1

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

Step-by-step 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 =
`-5^0C=(273-5)= 268K`

Number of moles (n) can be written as:

`n=(m)/(M)`

where, m = given mass

M = molar mass

`PV=(m)/(M)RT\\\\PM=(m)/(V)RT`

where,

`(m)/(V)=d`

where d = density

The relation becomes:

PM=dRT

`d=(PM)/(RT)`

`d=(1atm* 67.82g/mol)/(0.0821Latm/Kmol* 268K)=3.08g/L`

Thus the density of boron trifluoride gas is 3.08 g/L