the pressure of a gas depends in part on the average kinetic energy of its particles. this average kinetic…

the pressure of a gas depends in part on the average kinetic energy of its particles. this average kinetic energy is directly related to the gass temperature. the higher a gass temperature, the higher the average kinetic energy of its particles. if two gases have the same temperature, their particles have the same average kinetic energy. the statement below is about a gas in a closed, rigid container. click the blue words to correct the statement. if the temperature of the gas increases, the average kinetic energy of its particles increases. so, the gas will have a lower gas pressure.

the pressure of a gas depends in part on the average kinetic energy of its particles. this average kinetic energy is directly related to the gass temperature. the higher a gass temperature, the higher the average kinetic energy of its particles. if two gases have the same temperature, their particles have the same average kinetic energy. the statement below is about a gas in a closed, rigid container. click the blue words to correct the statement. if the temperature of the gas increases, the average kinetic energy of its particles increases. so, the gas will have a lower gas pressure.

Answer

Explanation:

Step1: Recall gas - pressure relationship

In a closed, rigid container, pressure is related to average kinetic energy.

Step2: Analyze effect of temperature on pressure

As temperature increases, average kinetic energy increases. Faster - moving particles collide more frequently and forcefully with the container walls. According to the ideal gas law (for a fixed volume and amount of gas, $P\propto T$), pressure increases.

Answer:

If the temperature of the gas increases, the average kinetic energy of its particles increases. So, the gas will have a higher gas pressure.