Question
Molar volume is the volume occupied by $1$ mol of any (ideal) gas at standard temperature and pressure: (STP: 1 atmospheric pressure, $0^\circ C$). Show that it is 22.4 litres.
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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 = $8.314J mol^{-1}K^{-1}$ n = Number of moles = 1 T = Standard temperature = 273K P = Standard pressure $= 1atm = 1.013 \times 10^5Nm^{-2}$
$\therefore\ \text {V}=\frac{\text{nRT}}{\text{P}}$
$=\frac{1\times8.314\times273}{(1.013\times10^{5})}$
$= 0.0224m^3 = 22.4$ litres Hence, the molar volume of a gas at STP is 22.4 litres.
$\therefore\ \text {V}=\frac{\text{nRT}}{\text{P}}$
$=\frac{1\times8.314\times273}{(1.013\times10^{5})}$
$= 0.0224m^3 = 22.4$ litres Hence, the molar volume of a gas at STP is 22.4 litres.
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