Equal masses of an ideal gas and a real gas having same molecular mass are placed in separate containers of equal volumes and at the same temperature. Which of the following will be the true statements ?

Molecules in ideal gas strike the walls with greater momentum than that in real gas

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The real gas exerts greater pressire than the ideal gas

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The real gas exerts lesser pressure than the ideal gas

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Free space available for the molecules to move about in real gas is smaller than that in ideal gas

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Solution

The correct option is D Free space available for the molecules to move about in real gas is smaller than that in ideal gas
In a real gas the molecules going to strike the walls of the container are attracted towards interior owing to the intermolecular forces. As a result the moleucules strike the walls with lesser momentum and exert lesser pressure than ideal gas.
Molecules in a real gas have finite size and occupy some volume. Thus the vacant (free) space available for the molecules to move about is somewhat decreased in comparision to ideal gas.

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