Molar volume is the volume occupied by $1 m o l$ of any (ideal) gas at standard temperature and pressure (STP : $1$ atmospheric pressure, $0^{o} C$ ). Show that it is $22.4 l i t r e s$ .

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Solution

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 $= 8.314 J m o l^{- 1} K^{- 1}$
n = Number of moles = 1
T = Standard temperature = 273 K
P = Standard pressure $=$ 1 atm $= 1.013 \times 10^{5} N m^{- 2}$
$∴ V = n R T / P$
$= 1 \times 8.314 \times 273 / (1.013 \times 10^{5})$
$= 0.0224 m^{3}$
$= 22.4$ litres
Hence, the molar volume of a gas at STP is 22.4 litres.

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

Molar volume is the volume occupied by $1 m o l$ of any (ideal) gas at standard temperature and pressure (STP : $1$ atmospheric pressure, $0^{o} C$ ). Show that it is $22.4 l i t r e s$ .