For the reactionCO(g) + Cl2(g) → COCl2(g)AG-71.4 kJ andAS-137.3 J/K at 269 K and 1 atm.This reaction is product favored under standard conditions at 269K.reactionThe standard enthalpy change for the reaction of 1.87 moles ofCO(g) at this temperature would be -1008.: kJ. For the reactionAH° =2H2S(g) + 302 (g) → 2H2O(l) + 2SO2(g)- 1124.0 kJ and AS° = -390.7 J/K==The standard free energy change for the reaction of 2.44 moles ofH2S(g) at 295 K, 1 atm would be 008.74 kJ.This reaction is product favored under standard conditions at 295K.Assume thatΔΗ° andorreactionAS are independent of temperature.

Answered: Image /qna-images/answer/51e4f85d-77b2-4dca-a1e1-e7fcd44bc05f.jpg

Answered: For the reaction CO(g) + Cl2(g) →…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 53QRT

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The value of G for the reaction 2C4H10(g)+13O2(g)8CO2(g)+10H2O(l) is 5490. kJ. Use this value and data from Appendix 4 to calculate the standard free energy of formation for C4H 10(g).
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
Thermite reactions have been used for welding metal parts such as railway rails and in metal refining. One such thermite reaction is Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(s). Is the reaction spontaneous at room temperature under standard conditions? During the reaction, the surroundings absorb 851.8 kJ/mol of heat.
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
One of the reactions that destroys ozone in the upper atmosphere is NO(g)+O3(g)NO2(g)+O2(g) Using data from Appendix 4, calculate G and K (at 298 K) for this reaction.
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)
Is the formation of ozone (O3(g)) from oxygen (O2(g)) spontaneous at room temperature under standard state conditions?
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
For the reaction SF4(g)+F2(g)SF6(g) the value of G is 374 kJ. Use this value and data from Appendix 4 to calculate the value of Gf for SF4(g).
Consider the reaction Fe2O3(s)+3H2(g)2Fe(s)+3H2O(g) a. Use Gf values in Appendix 4 to calculate G for this reaction. b. Is this reaction spontaneous under standard conditions at 298 K? c. The value of H for this reaction is 100. kJ. At what temperatures is this reaction spontaneous at standard conditions? Assume that H and S do not depend on temperature.
Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?
Using data from Appendix 4, calculate G for the reaction NO(g)+O3(g)NO2(g)+O2(g) for these conditions: T=298KPNO=1.00106atm,PO3=2.00106atmPNO2=1.00107atm,PO2=1.00103atm

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