Given: Half cell reaction                      E (V)  Ag+(aq) + e-  ---> Ag(s)         0.80 Cu+2(aq) + 2 e-  ---> Cu(s)     0.34 Zn+2(aq) + 2 e-  ---> Zn(s)    -0.76 Ni+2(aq) + 2 e-  ---> Ni(s)     -0.23   (a) Pick up two of the above listed half-cells to build a voltaic cell that would have a maximum overall cell potential. Write the overall reaction equation. (b) Draw a detailed cell diagram and indicate which electrode is anode and which is cathode, and indicate the (-) electrode and the (+) electrode.

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Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

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Q: Write the half-reactions as they occur at each electrode and the net cell reaction for this…

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Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A: The Relation between cell potential and free energy change is given by: Ecell can be determined from…

Q: Calculate AG° for the overall redox reaction: 2x3+(aq) + 2H2O(1) → H2O2(aq) + 2H*(aq) + 2x2+(aq)…

A: Gibbs energy delta G = -nFE.

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Q: In an electrolytic cell, Cu(s) is placed in the cathode half-cell while Ag(s) in the anode…

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Q: Consider the following standard reduction potentials. Reduction Half-Reaction Eo (volts) Cr3+(aq)…

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Q: 24. Given the following electrode (reduction) potentials: Fe3+ + e --> Fe2*; E° = 0.77 V Cu2* + 2e¯…

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Q: Calculate the standard state cell potential for the reaction below given the standard reduction…

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Q: (iv) Calculate the cell voltage for the reaction.

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Mno, (s) +…

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Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

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Q: A galvanic cell is powered by the following redox reaction: 2 I0, (aq) + 12 H"(aq) + 10 Cu*(aq) L(s)…

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Q: 20. A galvanic cell is constructed at 25°C as indicated in the shorthand cell notation: Determine…

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Q: A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential…

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Q: Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of…

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Q: Consider the standard reduction potentials and redox couples used in a galvanic cell. Unbalanced…

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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.