The heat of evaporation of liquid water at Ti=373K (boiling point) at the atmospheric pressure Pi=1bar is q(i)=41Kg/mol, the heat capacity of liquid water is p=10^3 Kg/m^3. Our goal is to find the enthalpy ?(f)H of the formation of water in it's standard (liquid) state at room temperature. T=298K. all gases in the problem are considered as ideal gases, the internal energy of ideal gas is given by U(T,V,n)=3/2nRT. Provide algebraic expression for all intermediate answers, you may provide a numerical value only for the final answer, i.e for the enthalpy ?(f) H of formation.

a)find the molar heat capacity Cp of liquid water in the proper unites J/(K mol)

b) Using the definition of enthalpy and the equation of state for ideal gas, find the molar enthalpy H(g) of water vapor at T(i) 373K and P(i)=1bar.

c) Using the first law of thermodynamic at constant volume or pressure (chose the relevant and explain why) find the molar enthalpy H of the liquid water at T(i)=373K and P(i)=1bar.

d)Using the relation between enthalpy and heat capacity at a constant volume or pressure (chose the relevant and explain why) fid the molar enthalpy H(p) of the liquid water at T(1)=298K and P(i)=1bar.

e) Find the enthalpy H(2) of the mixture of the molecular hydrogen and molecular oxygen in their standard gas state and the amount needed to produce 1mol of water via a chemical reaction a T(1) and P(i)=1bar.

f) Find the enthalpy delta H of the formation of liquid water in the standard state.

g) Find the value U of the molar internal energy of water at standard conditions.