Consider the following reaction:E2NO₂(g) N₂O4(9)->Type here to searchQWSEBiCRPart BFCalculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.38 atm and 1.63 atm, respectively.Express the free energy in kilojoules to two decimal places.AG= -6SubmitVΞΑΣΦhaxa xôx + √x √xxxProvide FeedbackPrevious Answers Request AnswerTPB1X1HX Incorrect; Try Again; 3 attempts remainingThis value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressutimes greater than that of the reactant, so the free-energy change is expected to be more positive than AG (Le., lesNGiven that AG-AG + RTIn Q, calculate the value of Q (it should be greater than 1 for the specified conditions)energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed insumming themLOWEO?MX.10nF20kJ490°F Clear

Gibbs free change of the reaction is to be calculated.

Consider the following reaction: 2NO₂(g) - N₂O4 (9) Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O, are 0.38 atm and 1.63 atm, respectively. Express the free energy in kilojoules to two decimal places. ΨΕ ΑΣΦ √√xx 1X1 ? X-10" 4

Consider the following reaction: 2NO₂(g) - N₂O4 (9) Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O, are 0.38 atm and 1.63 atm, respectively. Express the free energy in kilojoules to two decimal places. ΨΕ ΑΣΦ √√xx 1X1 ? X-10" 4

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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