Question

Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure (STP: 1 atmospheric pressure, 0 °C). Show that it is 22.4 litres.

Answer 1

Here,
Pressure P = 1 atm = 1.013 × 10^5 N/m² gas constant ( R) = 8.314 J/mol.K
number of mol ( n) = 1
Temperature ( T) = 273.15 K

Use ideal gas equation ,
PV = nRT
Put values of P, n , T and R
1.013 × 10^5 × V = 1 × 8.314 × 273.15
V = 8.314 × 273.15/1.013 × 10^5
= 0.0224 m³
= 22.4 L

Answer 2

Answer:

The ideal gas equation relating pressure (P), volume (V), and absolute temperature (T) is given as:

PV = nRT

Where,

R is the universal gas constant = 8.314 J mol–1 K–1

n = Number of moles = 1

T = Standard temperature = 273 K

P = Standard pressure = 1 atm = 1.013 × 105 Nm–2

∴ V = nRT / P

= 1 × 8.314 × 273 / (1.013 × 105)

= 0.0224 m3

= 22.4 litres

Hence, the molar volume of a gas at STP is 22.4 litres.