Please correct answer and don't used hand raiting and don't used Ai solution 12A solution of volume 50 cm³ contains 2.0 X 10°³ M Fe³+ and 1.0 X 10³ M³ 3Sn in 1MHC1. This solution is examined by voltammetry at a rotatingplatinum disk electrode of area 0.30 cm². At the rotation rate employed,both Fe 3+ and S n 4+ have mass-transfer coefficients, m, of 102 cm/s.(a) Calculate the limiting current for the reduction of Fe3+ under theseconditions, (b) A current- potential scan is taken from +1.3 to -0.40 Vvs. NHE. Make a labelled, quantitatively correct, sketch of the i-E curvethat would be obtained. Assume that no changes in the bulkconcentrations of Fe 3+ and S n 4+ occur during this scan and that allelectrode reactions are Nernstian

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Answered: 12 A solution of volume 50 cm³ contains…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.28QAP

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The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
At what pH does Ecell = 0.00 V for the reduction of dichromate by iodide ion in acid solution, assuming standard-state concentrations of all species except H+ ion?
How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
What is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
(a) Metals may be coated or plated for a number of reasons – state three reasons.(b) In an electroplating operation, what volume (cm3) and weight (g) of zinc will be deposited ontoa cathodic workpart if 10 A of current is applied for one hour? C = 4.75 x 10-2 mm3/A-s, cathodeefficiency E = 95%, density of zinc  = 7.15 g/cm3.
Use the References to access important values if needed for this question. A galvanic cell Cr(s)|Cr2+(aq) || Sn2+(aq)|Sn(s) is constructed using a completely immersed Cr electrode that weighs 24.5 g and a Sn electrode immersed in 638 mL of 1.00 M Sn2+(ag) solution. A steady current of 0.0416 A is drawn from the cell as the electrons move from the Cr electrode to the Sn electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Sn electrode gained when the cell is completely discharged? g (d) What is the concentration of the Sn2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M Submit Answer Try Another Version 2 item attempts remaining
For the reaction 3Cu(s) + 2Au3+(aq) 3Cu2+(aq) + 2Au(s), Eocell = 1.16 V. Calculate the cell potential when [Cu2+] = 0.54 M and [Au3+] = 0.042 M at 68.4oC.
5. For the following reaction at 25 °C, 5FE2+ *(aq) + MnO4 (aq) + 8H"(aq) = 5Fe*(aq) + Mn²*(aq) + 4H2O(1) calculate (a) the standard potential, (b) the equilibrium constant, and (c) the potential under these conditions: [Fe2+] = 0.50 M, [Fe³+] = 0.10 M, [MnO4 ]= 0.025 M, [Mn²*] = 0.015 M, and a pH of 7.00.
A galvanic cell is constructed that carries out the reaction 2 Ag(s) + Cl2 (g) 2 Ag* (aq) + 2 CI (ag) If the partial pressure of Clalg) is 1.00 atm, the initial concentration of Ag*(ag) is 0.25 M, and that of CI-(ag) is 0.016 M, calculate the initial voltage generated by the cell at 25°C.

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