(a) Find the equilibrium temperature that results when one kilogram of liquid water at 373-degrees K is added to two kilograms of liquid water at 283-degrees K in a perfectly insulated container. (b) When heat is added to or removed from a solid or liquid of mass m and specific heat capacity c, the change in entropy can be shown to be /S =mc ln(Tf/Ti), where Ti and Tf are the initial and final Kelvin temperatures. Use this equation to calculate the entropy change for each amount of water. Then combine the two entropy changes algebraically to obtain the total entropy change for the universe. Note that the process is irreversible, so the total entropy change of the universe is greater than zero. (c) Assuming that the coldest reservoir at hand has a temperature of 273-degrees K determine the amount of energy that becomes unavailable for doing work because of the irreversible process. Topic: Thermodynamics; Entropy and the Second Law of Thermodynamics.