Final answer:
An increase in gas particles and an increase in temperature would cause a higher frequency of collisions between gas particles and the walls of the container. However, the mass of the container and the volume of the container do not directly affect the frequency of collisions. option b is correct
Step-by-step explanation:
option b is correct An increase in gas particles will result in more collisions with the walls of the container, increasing the frequency of collisions. The force exerted by the particles on the walls will also increase. This can be observed through Avogadro's law, which states that at constant pressure and temperature, the frequency and force of molecule-wall collisions are constant. Therefore, scenario c, where more gas particles are introduced into the container, would cause a higher frequency of collisions with the walls of the container.
Additionally, an increase in temperature will cause the average speed and kinetic energy of the gas particles to increase. This leads to more frequent and forceful collisions with the walls of the container, as explained by Amontons's law. Thus, scenario b, where the temperature inside the container increases, would also result in a higher frequency of collisions.
On the other hand, scenarios a and d would not directly contribute to a higher frequency of collisions. The mass of the container (scenario a) does not affect the frequency of collisions between gas particles and the walls. Similarly, a decrease in the volume of the container (scenario d) does not directly affect the frequency, although it may increase the pressure exerted by the gas.