3.) Consider that the following half reaction is assigned a half cell voltage of0.00 V Hg (aq) +2 e Hg (1) E=0.00 V When this half-cell is paired with each of the following half-cells to form a complete cell in the laboratory, the following cell voltages are measured when the Hg cell is connected to the (+) terminal, thus acting as the cathode. Hg "Standard" Cell Potentials Ni/Ni*2 with Hg/Hg*2. 1.134 V Sn/Sn2 with Hg/Hg2. 0.99 V a. Calculate the reduction potentials using this Hg standard cell. V (Hg Standard) Ni*2 (aq) + 2 e → Ni(s) V (Hg Standard) Sn2 (aq) + 2 e Sn(s) 168

3.) Consider that the following half reaction is assigned a half cell voltage of0.00 V Hg (aq) +2 e Hg (1) E=0.00 V When this half-cell is paired with each of the following half-cells to form a complete cell in the laboratory, the following cell voltages are measured when the Hg cell is connected to the (+) terminal, thus acting as the cathode. Hg "Standard" Cell Potentials Ni/Ni2 with Hg/Hg2. 1.134 V Sn/Sn2 with Hg/Hg2. 0.99 V a. Calculate the reduction potentials using this Hg standard cell. V (Hg Standard) Ni*2 (aq) + 2 e → Ni(s) V (Hg Standard) Sn2 (aq) + 2 e Sn(s) 168

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.18QAP

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From the information provided, use cell notation to describe the following systems: (a) In one half-cell, a solution of Pt(NO3)2 forms Pt metal, while in the other half-Cell, Cu metal goes into a.Cu(NO3)2 solution with all solute concentrations 1 M. (b) The cathode consists of a gold electrode in a 0.55 M Au(NO3)3 solution and the anode is a magnesium electrode in 0.75 M Mg(NO3)2 solution. (c) One half-cell consists of a silver electrode in a 1 M AgNO3 solution, and in the other half-cell, a copper Electrode in 1 M Cu(NO3)2 is oxidized.
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.
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
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It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .