Calculate the changes in S and H for the processes of converting 1 mole of liquid water at 0◦C and 1 atm into steam at 200◦C and 3 atm. Assume water to have a constant density and a constant heat capacity of 4.18 kJ kg−1 K−1 . The enthalpy of vaporisation at 100◦C is 40.6 kJ mol−1 . Assume the steam to behave as an ideal gas and to have a heat capacity given by

cp= 8.81 − 1.9 × 10−3T + 2.2 × 10−6T 2

where cp is in cal K−1 mol−1 and T is in K