When considering the Ideal Gas equation of state, the molecules in the gas are a

Question

When considering the Ideal Gas equation of state, the molecules in the gas are assumed to have no interaction with each other at all. In real gases, however, attractive intermolecular forces exist between the molecules in the gas. The effect of these attractive intermolecular forces in a real gas is to:

(1) Decrease the size of the molecules in the gas.

(2) Decrease the pressure in the gas relative to that of an Ideal Gas

(3) Increase the volume of the gas relative to that of an Ideal Gas.

(4) Sometimes increase and sometimes decrease the pressure of the gas relative to an Ideal Gas.

(5) Decrease the temperature of the gas relative to that of an Ideal Gas.

*please also include reasoning as to why which one is the correct answer, thanks*

Explanation / Answer

Decrease the temperature of the gas relative to that of an Ideal Gas.

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