Direction: Solve the given problems involving Gibbs free Energy & Chemical Equilibrium. Write your answer on a separate sheet of paper. 2. Calculate AG° from standard enthalpy of formation and standard molar entropy values and predict whether the following reactions is spontaneous or not, at 25 °C. A. Haw + CO2 H2O + COu S° (J/mol.K) 130.6 213.6 188.8 197.9 AH? (kJ/mol) CO20 -393.5 -241.8 -110.5 B. FezO3w + 3H2 2Fe + 3H2O AH? (kJ/mol) S J/mol.K) Fe2O3 -822.2 90.0 130.6 Few H¿O 27.2 188.8 -241.8

Direction: Solve the given problems involving Gibbs free Energy & Chemical Equilibrium. Write your answer on a separate sheet of paper. 2. Calculate AG° from standard enthalpy of formation and standard molar entropy values and predict whether the following reactions is spontaneous or not, at 25 °C. A. Haw + CO2 H2O + COu S° (J/mol.K) 130.6 213.6 188.8 197.9 AH? (kJ/mol) CO20 -393.5 -241.8 -110.5 B. FezO3w + 3H2 2Fe + 3H2O AH? (kJ/mol) S J/mol.K) Fe2O3 -822.2 90.0 130.6 Few H¿O 27.2 188.8 -241.8

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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5. Calculate the standard entropy changes for the given reaction at 25°C. Use appendix 3 to determine the standard enthalpy of C, O2, and CO₂. C(graphite) + O₂(g) →>>> CO₂(g)
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18. Calculate AG at 298 K under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) Kp = 8.05 x 10ª P(CO) = 1.4 atm P(CO2) = 2.1 atm (R = 0.0821 atm.L/mol.K = 8.314 J/mol.K) * 2 Fe(s) + 3 CO29) %3D %3D %3D %3D +17.5 kJ/mol -25.0 kJ/mol O -30.7 kJ/mol +31.0 kJ/mol +2.99 kJ/mol
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For the reaction of gaseous substances with increasing gaseous molecules (from reactant to product side) and given the ΔH° that is +150 kJ/mol and ΔS° that is +171 J/K ∙ mol, how can you describe this reaction? a. It is spontaneous only at low temperatures. b. It is spontaneous only at high temperatures. c. It is spontaneous all the time. d. It is non-spontaneous.
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