Assertion : Compressibility factor for hydrog | vedclass

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Question

(A) For hydrogen gas $(H_2)$,the compressibility factor $Z$ is defined as $Z = \frac{PV}{nRT}$.For $H_2$,$Z$ is always greater than $1$ at all pressur

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If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.

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(A) For hydrogen gas $(H_2)$,the compressibility factor $Z$ is defined as $Z = \frac{PV}{nRT}$.For $H_2$,$Z$ is always greater than $1$ at all pressures,and it increases linearly with pressure.This indicates that the gas is more difficult to compress than an ideal gas,which is due to the dominance of repulsive forces between the molecules even at low pressures.Therefore,both the Assertion and the Reason are correct,and the Reason correctly explains the Assertion.

Assertion : Compressibility factor for hydrogen varies with pressure with positive slope at all pressures.
Reason : Even at low pressure,repulsive forces dominate hydrogen gas.

Similar Questions

At relatively high pressure,the van der Waals equation becomes?

Statement $-1$: The compressibility factor at the critical point is the same for different gases following van der Waal's equation.
Statement $-2$: The compressibility factor is independent of pressure at the critical temperature.

For a gas,the deviation from ideal behavior is maximum at:

What will the van der Waals equation be at high temperature and low pressure?

The compressibility factor $(Z)$ of a gas at moderate pressure is:

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Assertion : Compressibility factor for hydrogen varies with pressure with positive slope at all pressures.Reason : Even at low pressure,repulsive forces dominate hydrogen gas.