Imagine that you place a piece of copper with an initial temperature of 20°c in contact with some liquid water with an initial temperature of 100°c. assume that the physical system consisting of the copper and the water is thermally isolated from everything else; i. e., they can only exchange energy with each other. a) sketch two three-phase diagrams, one for each substance, and mark the initial state for each one. explain in a sentence or two how you can tell if either substance will undergo a phase change during the process of coming to thermal equilibrium. you do not need to do any calculations. b) construct a complete energy-system diagram for the process that ends when the two substances are in thermal equilibrium. don't forget that a complete diagram always includes an algebraic expression of energy conservation for parts (c) of this fnt use the same initial conditions for the copper, but assume that the h2o is initially in the gas phase at 100°c. sketch two three-phase diagrams, one for each substance, and mark the initial state for each one. how can you determine if the h2o will undergo a temperature change? what calculations and comparisons would you need to make? (don't actually do the calculations; just explain what you would need to do.)