Which of the following statements is true for real gases? Choose all that apply. As attractive forces between molecules increase, deviations from ideal behavior become more apparent at relatively low temperatures. Attractive forces between molecules cause an increase in pressure compared to the ideal gas. As attractive forces between molecules increase, deviations from ideal behavior become more apparent at relatively high temperatures. Attractive forces between molecules cause a decrease in pressure compared to the ideal gas.

Attractive forces between the gase molecules become significant at lower temperatures

Reason for that is when the temperature of the molecules decrease. the kinetic energy also decreases. at a certain low temperature the gases change into the liquid state. Therefore the attractive forces between these gas molecules become very significant near liquefying temperature. that's why they deviate from their original behavior at low temperature

Answer: Option (a) is the correct answer.

Explanation:

It is known that according to an ideal gas, there exists no force of attraction or repulsion between the molecules of a gas at low pressure and high temperature.

But in real gases, there exists force of attraction between tyhe molecules at low temperature. This is because at low temperature there occurs a decrease in kinetic energy of gas molecules due to which these molecules move slowly.

As a result, forces of attraction increases as molecules come closer to each other and therefore, gases deviate from an ideal gas behavior.

Therefore, we can conclude that the statement as attractive forces between molecules increase, deviations from ideal behavior become more apparent at relatively low temperatures, is true for real gases.