Question

1 a sample of oxy... volume of 2 l is compressed to a volume of 1 l. based on the kinetic theory of gases, how will the number of collisions and the pressure change when the volume of the gas is decreased? multiple - choice options with radio buttons, some text cut off

Explanation:

According to the kinetic theory of gases, when the volume of a gas is decreased (like compressing 2 L to 1 L), the gas particles are confined to a smaller space. So, the frequency of collisions between gas particles and with the container walls (number of collisions) increases. Also, pressure is related to the force of collisions per unit area. With more collisions and a smaller volume, the pressure increases. Among the options (assuming the correct option is the one where both number of collisions and pressure increase, likely the third option as per typical kinetic theory questions, but from the visible text, the option "The number of collisions and the pressure both increase" is the correct reasoning - as volume decreases, particle density increases, leading to more collisions and higher pressure due to more frequent wall impacts).

Answer:

The option (assuming the third option in the list, with text "The number of collisions and the pressure both increase"): The number of collisions and the pressure both increase.