The correct answer is option 3, which states that the kinetic energies of the gas molecules are higher at higher temperatures.

Gas molecules are in continuous motion, and their movement is characterized by kinetic energy. When the temperature of a gas increases, its molecules gain more kinetic energy. This increased kinetic energy leads to higher molecular velocities and more frequent collisions between molecules and the walls of the container.

As a result, the increased number of collisions and the higher velocity of the gas molecules exert a greater force on the walls of the container, leading to an increase in pressure. This relationship between temperature and pressure is explained by the kinetic theory of gases, which states that the pressure is directly proportional to the average kinetic energy of the gas molecules.

Options 1, 2, and 4 are not correct explanations for the increase in pressure with temperature. Gas molecules do not repel each other more, the potential energy of the molecules is not the primary factor influencing pressure, and gas molecules do not attract each other more at higher temperatures.

Therefore, the correct explanation is that the higher temperature increases the kinetic energies of the gas molecules, resulting in an increase in pressure.