PLEASE HELP The picture shows two containers filled with a gas, both initially at room temperature.
Which statement is correct? (5 points)
1) The average kinetic energy of the gas particles is greater in container A because its particles move faster.
2)The average kinetic energy of the gas particles is greater in container Bbecause it has a lower temperature.
3) The gas particles in both containers have the same average kinetic energy
because they have the same volume.
4)The gas particles in both containers have the same average kinetic energy
because they have equal number of particles.

The statement, average kinetic energy of the gas particles is greater in container A because its particles move faster is correct.

Explanation:

Kinetic energy is the energy obtained due to the motion of an object or substance.

where,

T = temperature

This means that kinetic energy is directly proportional to temperature.

So, when heat is provided to container A then its molecules will start to move rapidly from one place to another which will cause more collisions between the atoms.

Hence, average kinetic energy will be more in container A.

Whereas container B is placed at room temperature which is low than that in container A. So, molecules in container B will move at almost same speed and therefore, specific collisions will be there. So, average kinetic energy in container B will be less than that in container A.

Thus, we can conclude that the statement, average kinetic energy of the gas particles is greater in container A because its particles move faster is correct.

6.4 cm (max) - 25 cm (min)

c. electrical charges of ionic bonds.