Statement-1: Real gas approaches ideal gas be | vedclass

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(A) real gas behaves like an ideal gas when the intermolecular forces are negligible and the volume occupied by the gas molecules is negligible compar

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Statement-$1$ is True,Statement-$2$ is True; Statement-$2$ is a correct explanation for Statement-$1$.

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(A) real gas behaves like an ideal gas when the intermolecular forces are negligible and the volume occupied by the gas molecules is negligible compared to the total volume of the container.At low pressure,the molecules are far apart,making the intermolecular forces negligible.At high temperature,the kinetic energy of the molecules is high,which also makes the effect of intermolecular forces negligible.Thus,Statement-$1$ is True.At low pressure,the volume of the gas increases significantly for a given mass,which means the density $(\rho = m/V)$ becomes very low.This low density implies that the average distance between molecules is large,which justifies why the gas behaves ideally.Therefore,Statement-$2$ is True and is the correct explanation for Statement-$1$.

Statement-$1$: Real gas approaches ideal gas behaviour for low pressures and high temperatures.
Statement-$2$: At low pressure,the density of a gas is very low.

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Statement-$1$: Real gas approaches ideal gas behaviour for low pressures and high temperatures.Statement-$2$: At low pressure,the density of a gas is very low.