Answer to Question #115218 in General Chemistry for zainab

Question

A sealed container contains nitrogen gas. The pressure of the gas is due to the molecules of the gas hitting the walls of the container. Use the kinetic theory to explain why the pressure inside the container increases when the temperature is increased

Answer 1

According to the kinetic theory, the pressure of an ideal gas is equal to two-thirds of the average kinetic energy of the translational motion of the molecules contained in a unit volume.With increasing temperature, the kinetic energy of gas molecules increases, which will lead to an increase in pressure inside the container, gas molecules will hit the vessel walls more strongly.

The gas pressure on the vessel wall is due to the impact of molecules and with molecular - kinetic point of view is numerically equal to the collective the momentum they transmit per unit surface area per unit time. It is clear that the greater the kinetic energy of motion of each molecules, the greater the force arising from their impact on the wall. Besides the more molecules per unit volume n, the more often they hit her.