A standard voltaic cell is produced from half-cells (MnO4-/Mn*2, acidic medium) and (Fe/Fe2). What is the maximum work that can be provided by the standard cell? work = AG° = - z F E°cel- • Calculate answer in kilojoules units. • Write answer in 3 significant figures with the negative sign. • Do NOT write kJ anymore (example if calculated answer is -3.4567 kJ then final answer is -3.46. Standard reduction potential values: Mn04-/Mn*2: E° = +1.507 V Fe*3/Fe*2: E° = +0.771 V Use F= 96485 J/mol e- V

A standard voltaic cell is produced from half-cells (MnO4-/Mn2, acidic medium) and (Fe/Fe2). What is the maximum work that can be provided by the standard cell? work = AG° = - z F E°cel- • Calculate answer in kilojoules units. • Write answer in 3 significant figures with the negative sign. • Do NOT write kJ anymore (example if calculated answer is -3.4567 kJ then final answer is -3.46. Standard reduction potential values: Mn04-/Mn2: E° = +1.507 V Fe3/Fe2: E° = +0.771 V Use F= 96485 J/mol e- V

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 66QAP: Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C....

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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.
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?
What is the difference between and ? When is equal to zero? When is equal to zero? (Consider regular galvanic cells as well as concentration cells.)
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, .
Calculate E° for the following voltaic cells: (a) 2Na(s)+Fe2+(aq)2Na+(aq)+Fe(s) (b) 3SO42(aq)+12H+(aq)+2Al(s)3SO2(g)+2Al3+(aq)+6H2O (c) 2S(s)+4OH(aq)O2(g)+2S2(aq)+2H2O (basic)
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
Is it reasonable to conclude that a potential could be assigned to each half-cell in a voltaic cell, based on these data for three voltaic cells? Explain. Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s) cell potential=1.10 V Zn(s)|Zn2+(aq)||Ag+(aq)|Ag(s) cell potential=1.56 V Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s) cell potential=0.46 V
Why is a salt bridge necessary in galvanic cells like the one in Figure 17.4?
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi