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.
Carl works in a facility that keeps several gasses in tight containment units. He needs to monitor which gasses are under the most pressure for safety reasons. Each container has the same amount of gas in it. Containment Unit A is very hot to the touch, while Containment Unit B is cool to the touch.
Which containment unit should Carl be concerned with if he wants them to be at a low pressure?