In an experiment of a redox reaction, an electrochemical cell has been set up by connecting a vessel containing zinc, Zn metal being immersed in an aqueous solution of zinc ions, Zn2+ to another vessel of an aqueous solution containing a mixture of iron ions, Fe3+ and Fe2+ with platinum, Pt metal electrode. A wire and salt bridge are used to complete the circuit.Determine the new electrode potential, E cell if the concentration of Zn2+ solution is 0.35 M, while the concentrations of Fe3+ and Fe2+ solutions are adjusted to 0.50 M and 0.01 M, respectively.

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Q: Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these…

A: NOTE:  “Since you have posted a question with multiple sub-parts, we will solve first three subparts…

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A: Oxidation is the loss of electrons and reduction is the gain of electrons.

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Q: 1. (a) Balance the following simple redox reaction. Fe (s) + O₂(g) + 2H₂O (1)→ Fe³+ + 4 OH (b) If…

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Q: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

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Q: For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483…

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Q: Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction…

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Q: Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker…

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Q: Calculate the potential of a zinc electrode in a 0.0500 M solution of Zn (NO3) 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.