Determine E° for a galvanic (voltaic) cell if AG° = -6.3kJ/mol and n = 3. (F = 96,500 J/(V⚫ mol))Tap here or pull up for additional resources+

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Answered: Determine E° for a galvanic (voltaic)…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 29QAP: Calculate E° for the following voltaic cells: (a) MnO2+4H+(aq)+2I(aq)Mn2+(aq)+2H2O+I2(s) (b)...

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Similar questions

For a certain cell, G=25.0 kJ. Calculate E° if n is (a) 1(b)1(c) 41 Comment on the effect that the number of electrons exchanged has on the voltage of a cell.
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 cell reaction at 25°C where n=4 . Fill in the following table.
Consider a cell reaction at 25°C where n=2 . Fill in the following table.
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)
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
Consider a voltaic cell in which the following reaction takes place. 2F2+(aq)+H2O2(aq)+2H+(aq)2Fe3+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Calculate E at 25°C under the following conditions: [Fe2+]=0.00813M,[H2O2]=0.914M,[Fe3+]=0.199M,ph=2.88 .
Use the following half-equations to write three spontaneous reactions. Justify your answers by calculating E° for the cells. 1. MnO4(aq)+8H+(aq)+5eMn2+(aq)+4H2OE=+1.512V 2. O2(g)+4H+(aq)+4e2H2OE=+1.229V 3. Co2+(aq)+2eCo(s)E=0.282V
Calculate E° for the following voltaic cells: (a) MnO2+4H+(aq)+2I(aq)Mn2+(aq)+2H2O+I2(s) (b) H2(g)+2OH(aq)+S(s)2H2O+S2(aq) (c) an Ag-Ag+ half-cell and an Au-AuCl4- half-cell
For the standard cell potentials given here, determine the ?G for the cell in k].. (a) 0.000V,n=2 (b) +0.434V,n=2 (c) -2.439 V, n = 1
Sketch a galvanic cell, and explain how it works. Look at Figs. 17-1 and 17-2. Explain what is occurring in each container and why the cell in Fig. 17-2 works but the one in Fig. 17-1 does not.

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Determine E° for a galvanic (voltaic) cell if AG° = -6.3 kJ/mol and n = 3. (F = 96,500 J/(V⚫ mol)) Tap here or pull up for additional resources +