MnO4– + Sn ---> MnO2 + Sn2+ a) What is the half reaction that takes place at the cathode? b) What is the standard cell potential? c) What will be the potential of a cell constructed using 57.0 g MnO2, 1.57 M MnO4–, 14.8 g Pt, 12.5 g Sn and 0.87 M Sn2+ at pH 2.5?

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A: To calculate Standard potential , we use formula : E°cell =  E°r ( cathode ) - E°r (anode )

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Q: 10. Calculate the potential of the following cells: a) a galvanic cell consisting of a lead…

A: Given:  Pb2+ =0.0848 MZn2+=0.1364 M TiO2+ =0.00146 M Ti3+ =0.02723

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A: Given, Reaction : AgBr(s)+e-→Ag(s) +Br-(aq)       E°=0.070 V The Ksp value 5.4×10-13

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A: Given: [Mn3+ ] = 0.14 M [Mn2+ ] = 0.46 M [Sn2+ ] = 0.28 M And [Sn4+ ] = 0.056 M

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Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

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Q: Determine the cell potential and the equilibrium concentrations of the following concentration cell:…

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A: Nernst equation gives the relation between cell potential (Ecell), standard cell potential (Ecell°),…

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Q: When [Pb+1=1.01 M, the observed cell potential at 298 K for an electrochemical cell with the…

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Q: Use the References to access important values if needed for this question. Use standard reduction…

A: " Since you have posted multiple questions, we will provide the solution only to the first question…

Q: A student does an experiment to determine the molar solubility of lead(II) bromide. She constructs a…

A:

Q: Given a galvanic cell where one of the operating half reaction is: Pb (s) + 3 OH–(aq) ––––>…

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Q: 5) Calculate the cell potential for the following reaction that takes place in an electrochemical…

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Q: What is the cell potential for a cell with a 2.789 M solution of Zn2+ (aq) and 0.1408 M solution of…

A: We have to find cell potential for a cell with a 2.789 M solution of Zn2+ (aq) and 0.1408 M solution…

Q: n a Voltaic cell composed of CuôCu(NO3)2 and AgôAgNO3 half-cells, if the concentration of the…

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Q: 12.) The following cell is prepared and found to have a standard cell potential of 1.74 V: Pt (s)|Cl…

A: Cell representation:

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A: Given Ecell =0.189we know E°cell is 0 for hydrogen cell.

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A: Ca(s) + Cd2+(aq)  --> Ca2+(aq) + Cd(s)

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A: Given-> E°Ni2+/Ni = -0.25 V E°Co2+/Co = -0.28 V

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Q: The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn^2+(0.20 M)|| H+ (test solution)|…

A: Given, Cell potential = 0.475 V Temperature = 25°C =(25+273)K=298 K

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Q: a) Will the cell reaction proceed spontaneously as written for the following cell?    Sn (s)  |…

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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.