8. (I1.7) Using the following reactions at 298 K:CH,CHO + 2 H + 2e + CH;CH;OHE = -0.197 VNAD + H + 2e + NADHE = - 0.320 VCalculate the equilibrium constant for the first step in the metabolism of ethanol (CH,CH,OH) givenby the following reaction:CH,CH,OH + NAD' + CH,нО + NADH + H'9. (II.8) The dissociation constant (K) of a 0.010 M solution of a monoprotic acid at 298 K is1,47 x 10$. Calculate the percent dissociation (%) by using a mean activity coefficientY = 0.93.HA H + A

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8. (11.7) Using the following reactions at 298 K: CH,CHO + 2H + 2e CH,CH;OH E - -0.197 NAD + H + 2e NADH E®' = -0.320 V Calculate the equilibrium constant for the first step in the metabolism of ethanol (CH,CH,OH) given by the following reaction: CH,CH,OH + NAD' * CH,CHO + NADH + H’ (II.8) The dissociation constant (K) of a 0.010 M solution of a monoprotic acid at 298 K is 1,47 x 10%. Calculate the percent dissociation (%Au) by using a mean activity coefficient Ya = 0.93, НА * H + A

8. (11.7) Using the following reactions at 298 K: CH,CHO + 2H + 2e CH,CH;OH E - -0.197 NAD + H + 2e NADH E®' = -0.320 V Calculate the equilibrium constant for the first step in the metabolism of ethanol (CH,CH,OH) given by the following reaction: CH,CH,OH + NAD' * CH,CHO + NADH + H’ (II.8) The dissociation constant (K) of a 0.010 M solution of a monoprotic acid at 298 K is 1,47 x 10%. Calculate the percent dissociation (%Au) by using a mean activity coefficient Ya = 0.93, НА * H + A

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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2.4
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