Answer:
2.66 g/L
Explanation:
Data
[tex]Compound=N_2F_2[/tex]
[tex]T= 30\ºC\\T=(30+273)K=303K\\P=1atm[/tex]
As we have the compound we calculate the molar mass
[tex]N=14g/mol\\F=19g/mol\\M= 2(14)+2(19)=66 g/mol[/tex]
they tell us that [tex]N_2F_2[/tex] behaves like an ideal gas, therefore we can apply the equation of ideal gases
[tex]P.V=n.r.T\\r(constant of ideal gases)= 0.082\frac{atm.L}{K.mol}[/tex]
To apply this equation we lack several data, and within the variables of the equation there is no density that is what we need to find
But we can modify it in the following way so that it is based on the data we have
density formula
[tex]d=\frac{m}{V}[/tex]
from this formula we cleared the mass
[tex]d.V=m[/tex]
The formula for calculating moles is
[tex]n=\frac{mass(m)}{molar mass(M)}[/tex]
In this formula the mass also appears so we can substitute the variable mass for [tex]d.V[/tex]
[tex]n=\frac{d.V}{M}[/tex]
Replace in the equation of ideal gases, the variable mol (n) by [tex]\frac{d.V}{M}[/tex]
[tex]P.V=n.r.T\\P.V=\frac{d,V}{M}.r.T[/tex]
Now that we have the equation based on the data we have, we clear the density
[tex]P.V=\frac{d.V}{M}.r.T\\P.V.M=d.V.r.T\\[/tex]
As the volume appears on both sides of the equation we can simplify this term
[tex]\frac{P.M}{r.T}=d\\\\ \frac{1atm.66g/mol}{0.082atm.L/K.mol.303K}=d\\ \\2.66 g/L=d[/tex]
the density of dinitrogen difluoride gas at exactly 30 °C and exactly 1 atm is 2.66g/L
