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
Solution and Explanation
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
∴ \(V=\frac{nRT}{P}\)
\(=\frac{1×8.314×273}{1.013×10^5}\)
= 0.0224 m3
= 22.4 litres
Hence, the molar volume of a gas at STP is 22.4 litres.
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Concepts Used:
Behaviour of Real Gases
Real gases are gases that do not follow the ideal gas law, which assumes that gas particles have negligible volume and no intermolecular forces. In reality, gas particles do have volume and interact with each other, leading to deviations from ideal gas behavior.
The behavior of real gases can be described using various gas laws, such as the van der Waals equation and the virial equation. These equations take into account the effects of gas particle size and intermolecular forces on gas behavior.
One important property of real gases is compressibility. Real gases are more compressible than ideal gases, meaning that they can be compressed to a smaller volume at the same pressure. This is due to the fact that gas particles occupy a finite amount of space and are subject to intermolecular forces that can cause them to come closer together.
Also Read: Derivation from Ideal Gas Behavior
Another property of real gases is that their behavior is strongly affected by temperature and pressure. At high pressures and low temperatures, real gases tend to deviate more from ideal gas behavior. This is because the intermolecular forces become stronger and the gas particles are closer together.
Real gases also exhibit a phenomenon called condensation, where gas particles condense into a liquid or solid state when cooled or compressed sufficiently. This is due to the fact that the intermolecular forces become strong enough to overcome the kinetic energy of the gas particles, causing them to condense into a denser state.
Overall, the behavior of real gases is complex and influenced by various factors such as temperature, pressure, and intermolecular forces. Understanding the behavior of real gases is important in many scientific and industrial applications, such as in chemical reactions, power generation, and refrigeration.