An electrochemical cell utilizes the following redox reactionNHa * (ag) + 8Ce4"(ag) + зн-0() > NO; (ag) + 8Ce3"(ag) + 10н* (ag)Where the relevant half-reactions are:NO3 - (ag) + 1OH+ (ag) + 8e- → NH4 + (ag) + 3H20Ce**(ag) + e- > Ce3*(ag)Ecel = +0.88 VEcel = +1.72 V1. Calculate Ec(not under standard conditions) when [NH4 +1 = 0.35 M, [Ce**] = 0.25 M,[NO3 -1= 5.0 x10-2 M, [Ce3+] = 6.0 ×10-2 M, and the [H*] = 1.0 x10-3 M2. How is Ecel, impacted when the concentration of H* (ag) is reduced? In other words, whathappens when the pH decreases? Provide reasoning to support your answer.

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An electrochemical cell utilizes the following redox reaction NH4 + (ag) + 8Ce4*(ag) + 3H2O(I) → NO3- (ag) + 8Ce3*(ag) + 10H* (ag) Where the relevant half-reactions are: NO3 - (ag) + 10H* (ag) + 8e- → NH4 * (ag) + 3H2O Ce**(ag) + e- → Ce³*(ag) Ece = +0.88 V Ecel = +1.72 V 1. Calculate Ecu(not under standard conditions) when [NH4 1= 0.35 M, [Ce**] = 0.25 M, [NO3 -1= 5.0 x10-2 M, [Ce3+] = 6.0 ×10-2 M, and the [H*] = 1.0 x10-3 M

An electrochemical cell utilizes the following redox reaction NH4 + (ag) + 8Ce4(ag) + 3H2O(I) → NO3- (ag) + 8Ce3(ag) + 10H* (ag) Where the relevant half-reactions are: NO3 - (ag) + 10H* (ag) + 8e- → NH4 * (ag) + 3H2O Ce**(ag) + e- → Ce³*(ag) Ece = +0.88 V Ecel = +1.72 V 1. Calculate Ecu(not under standard conditions) when [NH4 1= 0.35 M, [Ce**] = 0.25 M, [NO3 -1= 5.0 x10-2 M, [Ce3+] = 6.0 ×10-2 M, and the [H*] = 1.0 x10-3 M

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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