30. Assuming that water vapor is an ideal gas with ν = 6,
calculate the following
for one mole:
(a) The enthalpy at 400 ◦C and 3 atm pressure;
(b) the enthalpy at 100 ◦C and 1 atm pressure;
(c) the enthalpy of one mole of liquid water at 100 ◦C and 1
atm pressure.
Hint: H = E + (pV), with E = Q − W; Q can be
obtained from the latent heat and W = pV is the work done
on
the water vapor by the atmosphere as its volume decreases from
the
gaseous to the liquid phase.
(d) Use the answer to part (c) and the specific heat of water
to find the
enthalpy at 50 ◦C and 1 atm.
(e) Use the answer to part (c) and the specific heat of water
to find the
enthalpy at 10 ◦C and 8 atm. (Liquid water is essentially
incompressible.)