MSE 3050, Phase Diagrams and Kinetics, Leonid Zhigileihomework #1 (page 1 out of 2)1. Calculate the molar enthalpy of pure iron at 1750 K and one atmosphere pressure.The molar heats of phase transformations for iron are: ΔHα→γ= 670 J/mol;ΔHγ→δ= 840 J/mol;ΔHδ→liquid= 13770 J/mol.The corresponding temperaturesof the phase transformations are: Tα→γ= 1187 K;Tγ→δ= 1664 K;Tδ→liquid= 1809 K.The constant pressure heat capacities of different phases of pure iron are:γ-Feα-Feδ-FecPα= 37.12 + 6.17×10-3T J/mol KcPγ= 24.47 + 8.45×10-3T J/mol KcPδ= 37.12 + 6.17×10-3T J/mol KcPliquid= 41.8 J/mol KMake a schematic plot of enthalpy vs temperature at one atmosphere pressure for pure iron in the temperature range from 298 K to 1750 K. In the plot, please use realistic scales for enthalpy and temperature. Show the values of enthalpies at T = 298 K, T = 1750 K, and at temperatures of all phase transformations that take place between 298 and 1750 K.MSE 3050, Phase Diagrams and Kinetics, Leonid Zhigileihomework #1 (page 2 out of 2)3. Calculate heat of formation of Al2O3 (the enthalpy change for oxidation reaction 2Al + 3/2 O2= Al2O3) at 1500 K. 4. An absent-minded cook left a pot with water on a hot stove. There are 4 liters of water in the pot and the stove supplies about 1 kJ/s to the water. When the cook left the kitchen, the water was at 50°C. How long it will take before all the water will be gone from thepot? Latent heat of vaporization of water is ΔHv= 2260 kJ/kg. You can assume a temperature-independent heat capacity of liquid water, Cp= 4.184 J/g K.You can use thermodynamic/thermochemical data given in tables at the end of the book by Gaskell or any other reliable and accessible source). Please give all the data and formulas used in calculations as well as references to the source of data.2. Calculate enthalpy of Al2O3at 3000 K. Assume a temperature-independent heat capacity in the liquid phase, Cpliquid= 192.5 J/mol