Calculate the change in entropy of 1.00 kg of water when it is heated from 10 degree c to 90 degree c. note: the specific heat capacity of water is 4186 j kg^-1 k^-1 given that the water was heated as a result of being added to an (otherwise) isolated heat reservoir at 90 degree c, what was the change in entropy of the heat reservoir, and what was the change in entropy of the complete system? how is the zeroth law of thermodynamics important in our definition of what temperature is? what does the first law of thermodynamics state? all process must abide by the first law of thermodynamics; however the first law of dynamics allows for some non-natural processes. give an example. the so called "central thermodynamic equation" states: tds = d e _ int + pdv show that this equation is consistent with the first law of thermodynamics. note any assumptions.