Question: I can use this background: Shown in the Figure below is a cylinder of gas on the left that is at room temperature (300 K). On the right, the cylinder has been heated until the Kelvin temperature has doubled to 600 K. The kinetic energy of the gas molecules increases, so collisions with the walls of the container are now more forceful than they were before. As a result, the pressure of the gas doubles. Decreasing the temperature would have the opposite effect, and the pressure of an enclosed gas would decrease.  Now, I have a new situation: A science teacher is attempting to show his students how kinetic energy works in gases. In order to do so, he leaves the classroom with two beakers filled with the same type of gas. He goes to the kitchen and heats one beaker up on the stove, but does nothing to the other beaker. He then returns to the classroom and has the students examine the gases. The students observe that the kinetic in beaker G is higher than that of the gas in beaker R.  Answer this question please: Which beaker did the teacher place on the stove?
Answer:
beaker G