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Consider a hypothetical gas which has the following Van der Waals constants:

a = 2.34 L2 bar mol-2

b = 0.0 L mol-1

Under conditions of very high pressures, what would you predict about the experimental volume of the gas?

The volume would be lower than predicted by the Ideal Gas Law

The volume would be higher than predicted by the Ideal Gas Law

The volume would be exactly the same as predicted by the Ideal Gas Law

Sagot :

Pstnonsonjokuidn

Under conditions of very high pressures, the volume would be lower than predicted by the Ideal Gas Law.

According to the kinetic theory of gases, a gas spreads out to fill the volume of the container holding it. Hence a gas does not have a definite volume due to the fact that there is no inter-molecular interaction between gas molecules.

When the gas is subjected to very high pressure, inter-molecular interactions become significant leading to a decrease in the volume of the gas.

Therefore, when subjected to high pressure, the experimental volume would be lower than predicted by the Ideal Gas Law.

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