3) Consider the following equilibrium: 2C0(g) = C(s) + CO2 (g)Thermodynamic data are provided in table given below:AH (kJ mol) S°(J K-mol-1)CO(g)C(s)CO2(g)-110.5197.95.69213.6-393.5You may assume that AH° and AS° do not vary with temperature.(a) Calculate the values of AH°rn and AS°,(b) At what temperature will an equilibrium mixture of 101.3 Pa total pressure contain the mixturein which partial pressure ratio of CO to CO2 is Pco/Pco2= 1/99? (R = 8.314 J/mol K)

Given: Total pressure = 101.3 Pa Pco/Pco2 = 1/99 R = 8.314 J/mol.K

3) Consider the following equilibrium: 2C0(g)= C(s) + CO2 (g) Thermodynamic data are provided in table given below: AH (k] mol-) S°J K-mol-1) CO(g) C(s) CO2(g) -110.5 197.9 5.69 213.6 You may assume that AH° and AS° do not vary with temperature. -393.5 (a) Calculate the values of AH°rn and AS°rxn (b) At what temperature will an equilibrium mixture of 101.3 Pa total pressure contain the mixture in which partial pressure ratio of CO to CO2 is Pco/Pco2 = 1/99? (R = 8.314 J/mol K) %3D

3) Consider the following equilibrium: 2C0(g)= C(s) + CO2 (g) Thermodynamic data are provided in table given below: AH (k] mol-) S°J K-mol-1) CO(g) C(s) CO2(g) -110.5 197.9 5.69 213.6 You may assume that AH° and AS° do not vary with temperature. -393.5 (a) Calculate the values of AH°rn and AS°rxn (b) At what temperature will an equilibrium mixture of 101.3 Pa total pressure contain the mixture in which partial pressure ratio of CO to CO2 is Pco/Pco2 = 1/99? (R = 8.314 J/mol K) %3D

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 94QAP: Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial...

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Similar questions

A process that is reactant-favored at equilibrium can never be spontaneous. This statement is (a) true (b) false
The free energy change, G, for a process at constant temperature and pressure is related to Suniv and reflects the spontaneity of the process. How is G related to Suniv? When is a process spontaneous? Nonspontaneous? At equilibrium? G is a composite term composed of H, T, and S. What is the G equation? Give the four possible sign combinations for H and S. What temperatures are required for each sign combination to yield a spontaneous process? If G is positive, what does it say about the reverse process? How does the G = H TS equation reduce when at the melting-point temperature of a solid-to-liquid phase change or at the boiling-point temperature of a liquid-to-gas phase change? What is the sign of G for the solid-to-liquid phase change at temperatures above the freezing point? What is the sign of G for the liquid-to-gas phase change at temperatures below the boiling point?
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial pressures of I2(g), H2(g), and HI(g) for the system 2HI(g)H2(g)+I2(g) at 500°C if the initial partial pressures are all 0.200 atm.
Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature. TiO2(s) + 3 C(s) 2 CO(g) + TiC(s) (a) Calculate rG and K at 727 C. (b) Is the reaction product-favored at equilibrium at this temperature? (c) How can the reactant or product concentrations be adjusted for the reaction to proceed at 727 C?
Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
The Haber-Bosch process for the production of ammonia is one of the key industrial processes in developed countries. N2(g) + 3H2(g) 2NH3(g) (a) Calculate rG for the reaction at 298 K, 800 K, and 1300 K. Data at 298 K are given in Appendix L Data for the other temperatures are as follows: How does the rG change with temperature? (b) Calculate the equilibrium constant for the reaction at 298 K, 800 K, and 1300 K. (c) At what temperature (298 K, 800 K, or 1300 K) is the mole fraction of NH3 the greatest?
When calcium carbonate is heated strongly, CO2 gas is evolved. The equilibrium pressure of CO2 is 1.00 bar at 897 C, and rH at 298 K is 179.0 kJ/mol-rxn. CaCO3(s) CaO(s) + CO2(g) Estimate the value of rS at 897 C for the reaction.
Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal moles of H2(g) at 1.00 atm and Br2(g) at 1.00 atm were mixed in a 1.00-L flask at 25C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique, and 1.10 1013 molecules were found. For this reaction, calculate the values of K, G, and S.