Okay, I am trying to work backwards from an exam which I messed up and I am trying to figure out what the lecturer did based on his answers posted online. Looking back, I realise one mistake I made was to use the specific heat of water given to calculate the enthalpy change in a transition from one pressure to the next.
In a transition within a Rankine cycle: I have P1 = P2 = 200 bar. Moving from 1 to 2, the water vapour turns to two-phase water and the enthalpy at point 2 is given as 2,353 kJ/kg. We also know that the enthalpy at 1 is 145 (worked out from a constant volume work problem and it checks out with the lecturer's answer).
Long story short: if I had tried to use the specific heat of water to determine the change in enthalpy and work from there to the enthalpy, I would have been way off. Instead, students were meant to use the given enthalpy value and then find the correct temperature from a table of saturated water provided.
I understand that the specific heat of water will change with temperature, but looking up the temperatures I am working at (changes from 30 C to 388 C) I can see that even an averaged out specific heat does not allow for a computation of a change in enthalpy from 145 to 2,353 (the second value was given). So I'm trying to figure out what I don't understand; why is a specific heat/temperature change calculation insufficient to calculate the enthalpy change here.