Question

Andre has a small glass with cold juice in it. He walks outside on a hot day, and places the glass on a table in front of his house. He has to go back in his house, forgets about his juice, and comes back outside after a few hours. Which statement is most likely to be true? A. The juice is at the same temperature as the air around it. B. The juice is losing heat to the air above it. C. The juice is losing heat to the glass around it. D. The juice is at a higher temperature than the glass surrounding it.

Answer 1

A

Step-by-step explanation:

This is due to thermal equilibrium. One system (the environment in this case) started out with a higher thermal state than the other system (the glass juice. Therefore there was an exchange of heat energy from the environment to the glass juice until the two systems attained a thermal equilibrium. This is in principle to the laws of thermodynamics, especially the second law on entropy.