Answer:
The density of nitrogen dioxide in a 3.50 L tank at 780.0 Torr and 37.0 °C is 1.86 g/L.
Explanation:
To calculate the density of gas, we use the equation given by ideal gas equation:
[tex]PV=nRT[/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] which is known as density of the gas
The relation becomes:
[tex]PM=dRT[/tex] .....(1)
We are given:
M = molar mass of argon = 46 g/mol
R = Gas constant = [tex]0.0821\text{ L atm }mol^{-1}K^{-1}[/tex]
T = temperature of the gas = [tex]27.0^oC=[37.0+273]K=310 K[/tex]
P = pressure of the gas = 780.0 Torr=[tex]\frac{780.0 }{760} atm=1.03 atm[/tex]
1 atm = 760 Torr
Putting values in equation 1, we get:
[tex]1.03 atm\times 46 g/mol=d\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 310 K\\\\d=1.86 g/L[/tex]
The density of nitrogen dioxide in a 3.50 L tank at 780.0 Torr and 37.0 °c is 1.86 g/L.
