my answer is wrong Calculate the pH of the cathode compartment for the following reaction given &= 3.01 V when [Cr³+ ] = 0.15 M, [A1³+ ]cell2-= 0.35 M, and [Cr₂0₂²- ] = 0.56 M.2-2 Al(s) + Cr₂0₂²¯(aq) + 14 H†(aq) → 2 Al³+ (aq) + 2 Cr³+ (aq) + 7 H₂O(l)0.94Enter a number.Need Help?Read ItWatch It

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Calculate the pH of the cathode compartment for the following reaction given & cell = 3.01 V when [Cr³+] = 0.15 M, [A1³+] = 0.35 M, and [Cr₂0₂²- ] = 0.56 M. 2 Al(s) + · Cr₂0₂²−(aq) + 14 H†(aq) → 2 Al³+ (aq) + 2 Cr³+ (aq) + 7 H₂O(1)

Calculate the pH of the cathode compartment for the following reaction given & cell = 3.01 V when [Cr³+] = 0.15 M, [A1³+] = 0.35 M, and [Cr₂0₂²- ] = 0.56 M. 2 Al(s) + · Cr₂0₂²−(aq) + 14 H†(aq) → 2 Al³+ (aq) + 2 Cr³+ (aq) + 7 H₂O(1)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 153CP: Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment...

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

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my answer is wrong

Calculate the pH of the cathode compartment for the following reaction given &
= 3.01 V when [Cr³+ ] = 0.15 M, [A1³+ ]
cell
2-
= 0.35 M, and [Cr₂0₂²- ] = 0.56 M.
2-
2 Al(s) + Cr₂0₂²¯(aq) + 14 H†(aq) → 2 Al³+ (aq) + 2 Cr³+ (aq) + 7 H₂O(l)
0.94
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