Part ADetermine A,G for the following reaction:2 NO(g) + 02(9) → N2O4(9)Use the following reactions with known AG" values:N,0,(9) + 2 NO, (g). A,G = 2.8 kJ mol-1NO(g) + 02(9) → NO2(9), A:G =. 36.3 kJ molExpress your answer using one decimal place.A,G° = -75.4 kJ molSubmitPrevlous AnewersCompletedPart BNow, calculate the A:G" for the same reaction, based on the Standard Gibbs Energies of formation:ArG"NO= 87.6 kJ - molArG N204 = 99.8 k.J - molTemplates Symbols undo redo feset keyboard shortcuts helpA,G° =kJ - mol

A) The reaction taking place is given as, => 2 NO (g) + O2 (g) ------> N2O4 (g) And the…

• Part A Determine A,G° for the following reaction: 2 NO(9) + O:(9) → N30«(9) Use the following reactions with known A,G° values: N;O,(9) → 2 NO,(9). A,G° = 28 kJ mol NO(9) + † O:(9) → NO;(9). A+G° = - 30.3 kJ mol Express your answer using one decimal place. 4,G- -75.4 kJ mol Submit Provioun Answere Completed • Part B Now, calculate the A-G° for the same reaction, based on the Standard Gibbs Energies of formation: A:GʻNO= 87.6 kJ - mol A:G°N;O4= 00.8 kJ - mol Tempianes Symdois uhdó rego tesét kayboard shortcuts Heip kJ- mol

• Part A Determine A,G° for the following reaction: 2 NO(9) + O:(9) → N30«(9) Use the following reactions with known A,G° values: N;O,(9) → 2 NO,(9). A,G° = 28 kJ mol NO(9) + † O:(9) → NO;(9). A+G° = - 30.3 kJ mol Express your answer using one decimal place. 4,G- -75.4 kJ mol Submit Provioun Answere Completed • Part B Now, calculate the A-G° for the same reaction, based on the Standard Gibbs Energies of formation: A:GʻNO= 87.6 kJ - mol A:G°N;O4= 00.8 kJ - mol Tempianes Symdois uhdó rego tesét kayboard shortcuts Heip kJ- mol

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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1. Calculate the ΔGf for the amino acid glycine at 339 K if the standard ΔGf = -378 kJ/mol and the standard ΔHf = -537 kJ/mol at 298 K. Assume ΔHf is constant over the temperature range. Ans. in 0 decimal places
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(Q70) Using the tabulated values from the text (located in Appendix G, beginning at p. 1211) calculate (and report in kJ) the standard Gibbs free energy (AG°rxn) for the net reaction that occurs during photosynthesis: 6 H2O (1) + 6 CO2 (g) --> C6H12O6 (s) + 6 O2 (g). The AG°; for glucose (C6H1206) is -1273.3 kJ/mol.
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