The compressibility of a gas is less than unity at STP. Therefore,
- $V_m > 22.4 L$
- $V_m < 22.4 L$
- $V_m - 22.4 L$
- $V_m = 44.8 L$
The Correct Option is B
Solution and Explanation
$\Rightarrow \, \, \, \, \, \, \, \, \, \, \, \, \, \, V < 22.4 L$
$\because \, \, \, \, \, \, \, \, \, \, \, V_{id}$(1 mol )=22.4 L at STP
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GMC Azamgarh Admission 2025: Dates, Courses, Fees, Eligibility, SelectJuly 22, 2025Concepts Used:
Van Der Waals Equation
Van der Waals equation is an equation relating the relationship between the pressure, volume, temperature, and amount of real gases.
Read More: Derivation of Van Der Waals Equation
Derivation of Van der Waals equation:
For a real gas containing ‘n’ moles, the equation is written as
Where, P, V, T, n are the pressure, volume, temperature and moles of the gas. ‘a’ and ‘b’ constants specific to each gas.
Where,
Vm: molar volume of the gas
R: universal gas constant
T: temperature
P: pressure
V: volume
Thus, Van der Waals equation can be reduced to ideal gas law as PVm = RT.
The equation can further be written as;
- Cube power of volume:
- Reduced equation (Law of corresponding states) in terms of critical constants:
Units of Van der Waals equation Constants
a: atm lit² mol-²
b: litre mol-¹