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: A. Decrease the size of the molecules in the gas B. Sometimes increase and sometimes decrease the pressure of the gas relative to an Ideal Gas C. Increase the Volume of the gas relative to that of an Ideal Gas D. Decrease the Temperature of the gas relative to that of an Ideal Gas E. Decrease the pressure in the gas relative to that of an Ideal Gas

Explanation / Answer

The pressure depends on the intensity of collisions with the walls, the change in pressure is related to the square of the number of molecules per volume of space, and thus for a fixed number of molecules, the change in pressure is inversely proportional to the square of the volume of the gas. The smaller the volume, the closer are the molecules and the greater will be the effect.

Thus, decreases the pressure in the gas relative to that of an ideal gas is the correct option.

Therefore, the correct option is E.

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