Question

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.

Explanation:

Step1: Recall gas - pressure relationship

In a closed, rigid container, according to the ideal gas law $PV = nRT$ (where $P$ is pressure, $V$ is volume, $n$ is the amount of gas, $R$ is the ideal - gas constant, and $T$ is temperature), when $V$, $n$, and $R$ are constant, $P$ is directly proportional to $T$.

Step2: Analyze the effect of temperature on pressure

Since the average kinetic energy of gas particles increases with temperature and the volume is constant (closed, rigid container), the gas particles collide more frequently and with greater force on the walls of the container. So, an increase in temperature leads to an increase in pressure.

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.