Six moles of chlorine gas at 273.15 K is placed into a 2.00L rigid, evacuated st

Question

Six moles of chlorine gas at 273.15 K is placed into a 2.00L rigid, evacuated steel cylinder tank. A student is asked to calculate the pressure using the Ideal Gas Law (PV=nRT) and determines the pressure to be 67.2 atm. The actual pressure gauge on the tank reads 55.0 atm. Which statement best explains the difference in the two pressures?

A) At this pressure, the gas has partially undergone deposition

B) The gas does bot behave as an ideal gas at that pressure due to its high density and intermolecular forces

C) At high pressure the volume of the gas particles needs to be taken into account

D) Chlorine is a diatomic molecule with twice the mass of a chlorine atom

Explanation / Answer

At high pressure and low temperature gases does not behave ideally. It happens becuase when the pressure is high then gas is compresed and it's molecules takes up some voluem and rest is free. So, when the pressure is very high and temperature is low then volume of gas particles must be takne into account.

hence, the correct choice is, (C).

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