Question

#1 please

INTRODUCTION TO GEOCHEMISTRY (GCH 3303) HOMEWORK #7 Due: March 28h, 2019 This homework is due at the start of class. If you wish to use this homework for studying for the second mid-semester exam, then make a copy of it before turning it in. Show all your work. No points will be given unless all work is shown. Standard conditions 298.15 K (25 °C) and 1 bar. Conversions Factors 1cal 4.184J Species/ Phase AHP (J mol)S° 1 bar 0.10J cm 1 atm 1.01325 bar 1 cm 0.10J bar 0°C 273.15 K Thermodynamic Data V° (em2 mol mol K-) 85.8 73.6 56.5 213.79 24.7892 L mol 56.5 69.91 MnCOs) Mn2+ Cl 31.073 21.0 17.3 -894.1 -220.75 -167.159 -393.509 -167.159 -285.83 17.3 18.068 Constants HCI R 83145 J mol' K-1 H00 Continuing with the carbonate reaction of Homework #5 MnCO, (s) + 2HC1-+ CO2(g) + H2O + 2Cr + Mn2+ Molar heat capacities in J mol K1 are 16.591 0.033026 -4.8117 x 10 -365.32 3399500 1. Calculate the entropy for the reaction at 500 °C 2. Calculate the reaction's equilibrium constant at standard conditions. 3. Calculate the equilibrium constant at 250 °C, using the van't Hoff equation. 4. Use the Clapeyron equation to calculate the slope of the phase boundary between the products and reactants. Make sure the units are bar K 5. Sketch a P-T diagram for the reaction. Label all appropriate components

Answer 1

The entropy change in a chemical reaction is given by the sum of the entropies of the products minus the sum of the entropies of the reactants.

Here m and n represents the coefficients in the balanced equation.

Lt CO 24 213.19 4 6 9.91 4 2 x 56.5 (-13.4)