A voltaic cell is constructed that uses the following half-cellreactions:Cu+(aq) + e- ----->Cu(s)I2(s) + 2 e- ----->2 I-(aq)The cell is operated at 298 K with [Cu+] = 0.25 M and[I-] = 0.035 M. (a) Determine E for the cell at these concentrations.(b) Which electrode is the anode of the cell?(c) Is the answer to part (b) the same as it would be if the cellwere operated under standard conditions? (d) If [Cu+] wereequal to 0.15 M, at what concentration of I- would the cellhave zero potential?

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A: The cell in which chemical energy is converted into electrical energy  is called Galvanic cell…

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A:

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A: E°cell = E°red(cathode)  -   E°red(anode)   ∆G°  =  -nFE°

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A: Given,                     AgCl s  +  e-  →  Ag s  +  Cl- aq                   E°red = 0.2223 V…

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A: The reaction: Ag+ + 1e- → Ag …..E◦ = 0.80 V Ni2+ + 2e- → Ni ….. E◦ =-0.23  V

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A: Here we are required to find the standard cell potential of the given electrochemical reaction.

Q: onsider a galvanic cell at T = 298K. F = 96 485C. the beginning (to), [Ca²+] = 0.01M, [H*] = 1M,…

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A:

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A:

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A:

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A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag 8° = +0.80 V Cd2+ + 2…

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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.