qeq380,EAH=-2855.4 kJ and AS = 92.7 J/KThe standard free energy change for the reaction of 1.71 moles of C₂H6 (g) at 319 K, 1 atm would beThis reaction isfavored under standard conditions at 319 K.Assume that AH and AS are independent of temperature.2C₂H6 (9)+702(g) → 4CO2 (g) + 6H₂O(g)CSubmit Answer$4RRetry Entire Group 9 more group attempts remainingShow Hint5TCengage Learning | Cengage Technical Support6BMacBook AirYH&7NU*81M(9KFO10PBPreviouskJ.Next>Save and Exit

Answered: Image /qna-images/answer/85d6f3b1-7394-4c8e-98c2-57d9178538aa.jpg

2C₂He (9)+702(g) → 4CO2(g) + 6H₂O(g) AH=-2855.4 kJ and AS = 92.7 J/K The standard free energy change for the reaction of 1.71 moles of C₂H6 (g) at 319 K, 1 atm would be This reaction is favored under standard conditions at 319 K. Assume that AH and AS are independent of temperature. kJ.

2C₂He (9)+702(g) → 4CO2(g) + 6H₂O(g) AH=-2855.4 kJ and AS = 92.7 J/K The standard free energy change for the reaction of 1.71 moles of C₂H6 (g) at 319 K, 1 atm would be This reaction is favored under standard conditions at 319 K. Assume that AH and AS are independent of temperature. kJ.

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...

See similar textbooks

Similar questions

Consider a chemical reaction where AS is 40.0 J/K, and AH is 25.0 kJ. What is the change in free energy (AG) for this reaction at 298K? O-22.4 kJ 3.9 kJ O 65.9 kJ O-37.9 kJ O 13.1 kJ
https://openstax.org/books/chemistry-atoms-first-2e/pages/g-standard-thermodynamic-properties-for-selected-substances a) Calculate ΔG° for the following reaction using the Standard Free Energy of Formation values. (SHOW CALCULATION) N2(g) + 3 F2(g) → 2 NF3(g) b) Is this reaction spontaneous or nonspontaneous?
For the reaction H₂S(g) + 2H₂O(1) → 3H₂(g) + SO₂(g) AH° = 295.4 kJ and AS 294.7 J/K The standard free energy change for the reaction of 1.91 moles of H₂S(g) at 333 K, 1 atm would be This reaction is ✓ favored under standard conditions at 333 K. Assume that AH° and AS° are independent of temperature. kJ.
A student determines the value of the equilibrium constant to be 1.21×106 for the following reaction.N2(g) + 3H2(g)2NH3(g)Based on this value of Keq:G° for this reaction is expected to be (greater,less) fill in the blank 1 than zero.Calculate the free energy change for the reaction of 2.01 moles of N2(g) at standard conditions at 298K. G°rxn = kJ
For the reaction CHĄ(g) + H,O(g)–→3H2(g) + CO(g) AH° = 206.1 kJ and AS° = 214.7 J/K %3D The standard free energy change for the reaction of 1.55 moles of CH,(g) at 320 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 320 K. Assume that AH° and ASº are independent of temperature.
33. Use the standard free energy of formation data in Appendix G to determine the free energy change for each of the following reactions, which are run under standard state conditions and 25 °C. Identify each as either spontaneous or nonspontaneous at these conditions. MnO2 (s) ⟶ Mn(s) + O2 (g) H2 (g) + Br2 (l) ⟶ 2HBr(g) Cu(s) + S(g) ⟶ CuS(s) 2LiOH(s) + CO2 (g) ⟶ Li2CO3 (s) + H2O(g) CH4 (g) + O2 (g) ⟶ C(s, graphite) + 2H2O(g) CS2 (g) + 3Cl2 (g) ⟶ CCl4(g) + S2Cl2 (g)
Using ONLY the information given in the problem (no thermodynamic table), calculate the standard free energy change for this reaction. At 298K, K = 6.74 x 106 for the following reaction: %3D C;H,O3 (g) C,H6(g) + 3CO(g)
A student determines the value of the equilibrium constant to be 2.30 x 10¹6 for the following reaction. Ca(OH)2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(1) Based on this value of Keq AGO for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 1.57 moles of Ca(OH)2 (aq) at standard conditions at 298 K. AGO rxn kJ
[Review Topics] [References] Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.21x1012 for the following reaction. CO(g) + Cl2(g)- COC12(g) Based on this value of Keg AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.65 moles of CO(g) at standard conditions at 298K. AG rxn kJ
Calculate standard free energy change using AGf values. Consider the reaction 2NH3(g) + 3N₂O(g)4N₂(g) + 3H₂O(g) Use standard free energies of formation to calculate the standard free energy change for this reaction at 25°C. kJ/mol AG° = rxn
For the reaction CH4 (9) + H₂O(g) → 3H₂(g) + CO(g) AH = 206.1 kJ and AS = 214.7 J/K The standard free energy change for the reaction of 1.83 moles of CH4 (9) at 345 K, 1 atm would be kj. This reaction is favored under standard conditions at 345 K. Assume that AH and AS are independent of temperature.
For the reaction CO(g) + 3H₂(g) → CH4 (9) + H₂O(g) ΔΗ° - 206.1 kJ and AS = - 214.7 J/K The standard free energy change for the reaction of 1.67 moles of CO(g) at 253 K, 1 atm would be This reaction is favored under standard conditions at 253 K. Assume that AH° and AS° are independent of temperature. == kJ.