Question

The density of no2 in a 4.50 l tank at 760.0 torr and 25.0 °c is ________ g/l.

Answer 1

From  ideal  gas  equation   that   is   PV=nRT
n(number of  moles)=PV/RT
P=760 torr
V=4.50L
R(gas  constant =62.363667torr/l/mol
T=273 +273=298k
n  is   therefore   (760torr x4.50L) /62.36367 torr/L/mol  x298k  =0.184moles
the  molar  mass  of  NO2 is  46  therefore  density=  0.184  x  46=8.464g/l

Answer 2

Answer:

The nitrogen dioxide gas is 4.43 g/L.

Explanation:

Pressure of the of the gas = P = 760.0 torr = 2.356 atm

(1 torr = 0.00131 atm)

Volume of the tank = 4.50 L

Temperature of the gas = 25 °C = 298 K

Moles of gas = n = $\frac{mass}{46 g/mol}$

Using an ideal gas equation:

$PV=nRT$

$\frac{P\times 46 g/mol}{RT}=\frac{Mass}{V}=Density$

$Density=\frac{2.356 atm\times 46 g/mol}{0.0820 L atm/mol K\times 298 K}$

Density = 4.43 g/L

The nitrogen dioxide gas is 4.43 g/L.