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:

According to the given information, the pressure of a gas depends on the average kinetic energy of its particles, and the average kinetic energy is directly related to temperature. When temperature increases, average kinetic energy increases. In a closed, rigid container (volume \(V\) is constant), from the ideal - gas law \(PV = nRT\) (where \(P\) is pressure, \(n\) is the amount of gas, \(R\) is the gas constant, and \(T\) is temperature), when \(V\), \(n\), and \(R\) are constant, \(P\propto T\). So when \(T\) (and thus average kinetic energy) increases, pressure should increase, not decrease.

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.