What is the density of laughing gas, dinitrogen monoxide, n2o, at a temperature of 325 k and a pressure of 113.0 kpa?

Answer : the density of the N₂O at 325 K and 113.0 kPa is 1.84 kg m⁻³.

Explanation:

Density (kg/m³) = mass (kg) / Volume (m³)

d = m/V (1)

Ideal gas law,

PV = nRT (2)

Where, P is the pressure of the gas (Pa), V is the volume of the gas (m³), n is the number of moles of gas (mol), R is the universal gas constant (8.314 J mol ⁻¹ K⁻ ¹) and T is temperature in Kelvin.

n = m/M (3)

Where, n is number of moles, m is mass and M is molar mass.

From (2) and (3),

PV = (m/M) RT

By rearranging,

P = (m/VM) RT (4)

From (1) and (4)

P = (dRT) / M

The given data,

P = 113.0 kPa = 113.0 x 10 ³ Pa

d = ?

R = 8.314 J mol ⁻¹ K⁻ ¹

T = 325 K

M = 44.0 g/mol = 44.0 x 10⁻³ kg/mol

By substitution,

113.0 x 10³ Pa = (d x 8.314 J mol⁻¹ K⁻¹ x 325 K) / 44.0 x 10⁻³ kg/mol

d = (113.0 x 10³ Pa x 44.0 x 10⁻³ kg/mol) / (8.314 J mol⁻¹ K⁻¹ x 325 K)

d = 1.84 kg m ⁻ ³

Hence, the density of the N ₂O at 325 K and 113.0 kPa is 1.84 kg m⁻³.

Assumption made is "N ₂O gas has an ideal gas behavior".