The key principle is the ideal gas law (PV = nRT or PV = NkT, where N is the number of particles and k is Boltzmann's constant). The pressure of an ideal gas depends only on the number of particles, volume, and temperature, not on the type of gas (as long as it behaves ideally). Since the number of particles is halved while temperature and volume are kept constant, the pressure must also be halved.
A stainless steel chamber contains Ar gas at a temperature T and pressure P. The total number of Ar atoms in the chamber is n. Now Ar gas in the chamber is replaced by CO₂ gas and the total number of CO₂ molecules in the chamber is n/2 at the same temperature T. The pressure in the chamber now is P'. Which one of the following relations holds true? (Both the gases behave as ideal gases)
Asked in UPSC NDA 2 2018 · Topic: Heat and Thermodynamics (Kinetic Theory of Gases (Assumptions, Pressure, Temperature, Ideal Gas Equation))
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