please help me with the gas laws in chemistry

Question

Which of the following is true if the temperature of the gas in a cylinder is increased, while the number of moles of gas and volume of the container remains the same? Select all that apply.

A. molecules move faster

B. molecules move slower

C. kinetic energy increases

D. kinetic energy decreases

E. collisions on the walls of container increases

F. collisions on the walls of container decreases

G. pressure increases

H. pressure decreases

Select all that are correct

Answer 1

For this question, we first need to consider the definition of temperature.

Temperature is the average kinetic energy of all the particles in the system. In other words, the kinetic energy can be written as (sum of all kinetic energies) divided by (total number of particles).

Since the volume and moles (or quantity) of particles is staying constant, while the temperature is increasing, the molecules must be moving faster. This is because when the total number of particles is staying the same (moles), the kinetic energies must be increasing for the temperature to increase. This means that the kinetic energy of the system is increasing and the speed of particles is increasing (since kinetic energy increases with an increase in the speed of the particles).

When the molecules are moving faster in a confined space, the collisions on the walls of the container also increases. This is because as particles are moving faster, they are hitting the walls of the container more often and colliding with other particles more often.

To consider pressure, we must look at the ideal gas law PV = nRT.

According to the ideal gas law, when temperature increases, the pressure also increases when volume and moles of gas are constant. To see this we can rearrange PV = nRT to P/T = nR/V. As P or pressure increases, temperature must increase as well since nR/V is staying constant.

Therefore, A, C, E and G are correct.