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

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 78E: Consider the following reaction at 298 K: 2SO2(g)+O2(g)2SO3(g) An equilibrium mixture contains O2(g)...

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Similar questions

Consider the reaction CO(g)+H2O(g)CO2(g)+H2(g) Use the appropriate tables to calculate (a) G at 552C (b) K at 552C
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
For each reaction, an equilibrium constant at 298 K is given. Calculate G for each reaction. (a) Br2()+ H2(g)2HBr(g) KP = 4.4 1018 (b) H2O()H2O(g) KP = 3.17 102 (c) N2(g) +3H2(g)2NH3(g) Kc = 3.5 108
A process that is reactant-favored at equilibrium can never be spontaneous. This statement is (a) true (b) false
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?
Consider the following reaction at 298 K: 2SO2(g)+O2(g)2SO3(g) An equilibrium mixture contains O2(g) and SO3(g) at partial pressures of 0.50 atm and 2.0 atm, respectively. Using data from Appendix 4, determine the equilibrium partial pressure of SO2 in the mixture. Will this reaction be most favored at a high or a low temperature, assuming standard conditions?
Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
Hydrogenation, the addition of hydrogen to an organic compound, is an industrially important reaction. Calculate rH, rS, and rG for the hydrogenation of octene, C8H16, to give octane, C8H19 at 25 C. Is the reaction product- or reactant-favored at equilibrium? C8H16(g) + H2(g) C8H18(g) Along with data in Appendix L, the following information is needed for this calculation.
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.
Given the following data at 25C 2NO(g)N2(g)+O2(g)K=1 10 30 2NO(g)+Br2(g)2NOBr(g)K=8 101 Calculate K for the formation of one mole of NOBr from its elements in the gaseous state.
Elemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2. BCl3(g) + 3/2 H2(g) B(s) + 3HCl(g) Calculate H, S, and G at 25 C for this reaction. Is the reaction predicted to be product favored at equilibrium at 25 C? If so, is it enthalpy driven or entropy driven?

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