The standard molar entropies of water ice, liquid and vapor are 37.99, 69.91, and 188.83 J K-1mol-1, respectively. On a single graph, show how the Gibbs energies of each of these phases vary with temperature between – 20 C and 150 C for a constant pressure of 80 kPa. You can start your computations at the triple point (pressure of 0.611 kPa and temperature of 0.01 C) where the molar Gibbs energy of all three phases are equal and can be assigned an arbitrary value of 1000 J mol-1. Use a molar volume of liquid water of 0.018 L mol?1 and solid water of 0.0195 L mol?