Answer:
D.)more collisions --> greater collision force --> higher pressure
Explanation:
The temperature of an ideal gas is directly proportional to the average kinetic energy of the particles in the gas, according to the equation:
[tex]KE=\frac{3}{2}kT[/tex]
where
KE is the kinetic energy
k is the Boltzmann's constant
T is the absolute temperature of the gas
As a result, when the temperature of a gas increases, the kinetic energy of the particles increases too. This means that overall, they will move faster, therefore there will be more collisions between the particles and the walls of the container. As a result, the particles will exert on average a greater force of collision agains the walls, and therefore, they will exert a higher pressure.
So, the correct option is
D.)more collisions --> greater collision force --> higher pressure
Answer:
its A
Explanation:
Found it on quizlet "topic test 6 topic review activity"
