You need to compute the molar Gibbs energy for ice, liquid and vapor for water for temperaturesvarying between – 50 C and 150 C at a pressure of 80 kPa. You can start your computations atthe triple point (pressure of Pi=0.611 kPa and temperature of Ti=0.01 C) where the molar Gibbsenergies of all three phases are equal and can be assigned an arbitrary value of 1000 J mol-1.First, compute the molar Gibbs energy for each phase for a pressure of Pf=80 kPa (from initialpressure of 0.611 kPa) and a constant temperature of 0.01 C. Use a molar volume of liquid waterof 0.018 L mol‐1 and solid water of 0.0195 L mol‐1. Second, at a constant pressure of 80 kPa,compute the molar Gibbs energy for each of the phase for temperatures varying between – 50 CBatteryElectrical Work2 2 O2 21 H O H H2 O2 Bruce N. Wilson Chapter 5: Supplemental MaterialsLast Modified: April, 2016 5s-2 Biological and Environmental Thermodynamicsand 150 C. Standard molar entropies of water ice, liquid and vapor are 37.99, 69.91, and 188.83J K-1mol-1, respectively. On a single graph, plot the molar Gibbs energy of each phase withtemperature. Identify the range of temperatures corresponding to ice, liquid and vapor. What isthe freezing point and boiling point temperatures (these correspond to P = 80 kPa)? It isrecommended that you solve this problem using spreadsheets with temperature varying in 5 Cincrements.
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