Question

The density of no2 in a 3.50 l tank at 780.0 torr and 37.0 °c is __________ g/l.

Answer 1

We assume that the given gas, NO2, is an ideal gas such that we will be able to use the equation,
                          n/V = P/RT
where n is the number of moles, V is volume, P is pressure, R is gas constant, and T is temperature in kelvin. Substituting the known values,
                        n/V = (1 atm) / (37 + 273)(0.0821 L.atm/mol.K)
                                       n/V = 0.039 mol/L
Converting this to density by multiplying the value with the molar mass,
                               density = (0.039 mol/L) x (46 g/mol) = 1.8 g/L

Answer 2

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:

$PV=nRT$

Number of moles (n)

can be written as: $n=\frac{m}{M}$

where, m = given mass

M = molar mass

$PV=\frac{m}{M}RT\\\\PM=\frac{m}{V}RT$

where,

$\frac{m}{V}=d$ which is known as density of the gas

The relation becomes:

$PM=dRT$    .....(1)

We are given:

M = molar mass of argon = 46 g/mol

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature of the gas = $27.0^oC=[37.0+273]K=310 K$

P = pressure of the gas = 780.0 Torr=$\frac{780.0 }{760} atm=1.03 atm$

1 atm = 760 Torr

Putting values in equation 1, we get:

$1.03 atm\times 46 g/mol=d\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 310 K\\\\d=1.86 g/L$

The density of nitrogen dioxide in a 3.50 L tank at 780.0 Torr and 37.0 °c is 1.86 g/L.