4. The cell potentials of many oxidation-reduction reactions are highly dependent on pH. Consider the following equation: 3 Co(s) + 2NO3(aq) + 8 H+ (aq) -----> 3 Co2+ (aq) + 2NO(g) + 4H₂O(1) a) Determine the standard cell potential for the reaction. b) What would be the pH of the solution at standard conditions? (HINT: What are the concentrations of all aqueous species at standard conditions?) c) Determine the cell potential for the reaction at a pH of_2.0. (Hint: You will need to use the Nernst equation.) Assume that all concentrations, other than that of H*, are standard. d) Based on your answers above, would you say that the reaction is more favorable (i.e., more spontaneous) at higher pH or lower pH? Explain.

Q: 3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of…

A: Given cell reaction: 3Co(s)+2NO3-(aq)+8H+→3Co+2(aq)+2NO(g)+4H2O(l)

Q: Physical constants that you may need: R = 8.31446 mol K C Faraday's constant F= 96485 mol e Gas…

A: Using Nernst's equation, pH of the solution can be determined from Ecell.

Q: Given the standard cell potential, E°ce = 1.10 V, for the cell, Zn(s) | Zn(NO,)(aq) || Cu(NO,)(aq) |…

A: Standard cell potential (E°cell) = 1.10 V  Temperature = 25°C.  The reaction :  Zn(s) + Cu2+(aq)…

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Q: The standard cell potential for the following galvanic cell is 0.390 V.  What is the cell potential…

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A: Given: Cell reaction: Sn2+(aq) + Ba (s)---> Ba2+(aq) + Sn (s)

Q: The standard cell potential for the following galvanic cell is 0.390 V.  What is the cell potential…

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A: Given : Table of half reactions and reduction potential.  To find: Complete the given table.…

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A: We have find out the PH of unknown solution at 298 K.

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Q: Consider the following reaction and its AG° at 25.00 °C. Fe2+ (aq)+Zn(s) → Fe(s) + Zn²*(aq) AG° =…

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Q: For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777…

A: Ecell = 0.3657 V PH2 = 0.777 atm The balanced reduction half reactions  2 H+ (aq) + 2 e- ----->…

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Q: Consider the following electrochemical cell:…

A: In electrochemical cell redox reaction occur

Q: The following galvanic cell has 8° = +1.887 V at 25°C: Co(s) | Co2+ (aq) || Ce4+ (aq), Ce3+ (aq) |…

A: The solution is as follows:

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au*(aq) =…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

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Q: For the cell shown, the measured cell potential, Ecell, is -0.3725 V at 25 °C. Pt(s) | H₂(g,0.849…

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Q: 1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V,…

A: Calculate the cell potential of the given galvanic cell.  Given  At Anode  Cu/Cu2+; E°=-0.34 V At…

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A:

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.