The standard cell potential (at 298 K) for the Daniell cellvalues of AG andis 1.10 V. Calculate the correspondingK and comment on the thermodynamic viability of thecell reaction:Zn(s) + Cu²+ (aq) -Zn²+ (aq) + Cu(s)(F= 96 485 C mol¹; R = 8.314 x 10³ kJ K-¹ mol-¹)The equation needed is:AG=-zFE celland z is 2 for the cell reaction:Zn(s) + Cu²+ (aq) → Zn²+ (aq) + Cu(s)AG = -zFE cell= -2 x 96485 × 1.10= -212 267 J per mole of reaction≈-212 kJ per mole of reactionIn K ==AG°RT-2128.314 x 10-3 × 298In K = 85.6K = 1.50 × 10³7The large negative value of AG° and a value of K which is>>>1 correspond to a thermodynamically favourable reaction,one which virtually goes to completion.3. At 298 K, E cell for the Daniell cell is 1.10 V. Determinethe equilibrium ratio [Cu²+]/[Zn²+].[Ans. 6.90 × 10 387

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Answered: 3. At 298 K, E cell for the Daniell…

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3. At 298 K, E cell for the Daniell cell is 1.10 V. Determine the equilibrium ratio [Cu²+]/[Zn²+]. [Ans. 6.90 × 10 38]

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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