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Intermolecular forces are the forces that exist between molecules. These forces can affect the properties of a substance, including its phase, solubility, and boiling and melting points. In gases, the intermolecular forces are typically weak compared to solids and liquids, because gas particles are farther apart from one another. However, when the conditions change, these forces can become more significant.

When a gas is compressed to a smaller volume at constant temperature, the particles are forced into a smaller space and become closer together. This results in an increase in the frequency and strength of intermolecular collisions/interactions. Consequently, the effect of intermolecular attraction becomes more significant as gas is compressed. The gas particles are now close enough to feel each other's presence, and their motion may be influenced by the attractive forces between them. This will lead to deviation from the ideal behavior (predicted by the Ideal Gas Law) and the gas will exhibit more "real" behavior.

In the case where temperature is increased while keeping the volume constant, the average kinetic energy of the gas particles also increases (since temperature is proportional to the average kinetic energy). This means the particles are moving faster and the collisions between them become more energetic. Since the intensity of intermolecular forces depends on the distance between particles (it decreases with the increase in distance), the increase in the temperature causes a decrease in the intermolecular force due to the higher energy of the particles, which leads to more distance between them. As a result, the effect of intermolecular attraction becomes less significant when the temperature of the gas is increased at a constant volume. The gas will act more like an ideal gas and less like a "real" gas.