Calculate to three significant digits the density of boron trifluoride gas at exactly 20 c and exactly 1atm . you can assume boron trifluoride gas behaves as an ideal gas under these conditions.

0.5583  g/L[/tex]

Explanation:

Since boron trifluoride ( B ) Is an ideal gas , we can apply IDEAL GAS EQUATION which is ,

PV  = nRT

Where ,

P - the pressure at which it is present (20 atm)

V - volume of the gas (needed)

n - number of moles of the gas taken (1 mol)

R - universal gas constant which is 8.314

T - temperature of the gas ( 273 + 20 = 298 K )

thus ,

density ρ =

mass of  B is :

B : 11

F : 19

therefore , mass = 11 +

=68 g

density =

the answer is option a.