Question

The picture shows two containers filled with a gas, both initially at room temperature.
Room Temperature A Heat B
Which statement is correct?
A) The average kinetic energy of the gas particles is greater in container A because its particles move faster.
B) The average kinetic energy of the gas particles is greater in container B because it has a lower temperature.
C) The gas particles in both containers have the same average kinetic energy because they have the same volume.
D) The gas particles in both containers have the same average kinetic energy because they have equal number of particles.

Answer 1

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

What is the relation between temperature & kinetic energy?

Kinetic energy of any particle is directly proportional to the temperature of the sample of that particle.

From the given diagram, it is clear that:

• In beaker A, heat is supplied to the beaker due to which temperature of the beaker A increases as a result of it particles of gases will move with faster velocity because kinetic energy of the gases particle increases.
• Beaker B is present at room temperature, so particles in this beaker will have less velocity as compared to beaker A.

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

To know more about average kinetic energy, visit the below link:
https://brainly.com/question/14432752

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