Consider the following electrochemical cell:Pt|H2(g,p°)|HCI(aq,b)|Hg2Cla(s)[ Hg(1)The potential of this cell, in relation to different molalities (b), has been measured with high precision at25°C. The following results have been obtained:b/mmol.kgE/VI (ionic strength)Y: (DHLL)Y+ (linear fit)1.60773.07695.04037.693810.94740.600800.568250.543660.522670.50532(i)Write the half-reactions for the cell, and show the standard potential of each half-reaction.(ii)(ii) Write the cell reaction for this cell.(iv) Write the Nernst equation for this cell in terms of molality (b) and the mean activity coefficient (ya) ofDetermine the standard cell potential through simple calculation.HCI.(v) Determine the ionic strength (1) for each molality (b) (and complete the above table).(vi) By employing the Debye-Hückel limiting law (DHLL), determine the mean activity coefficient (y4) of HCI(and complete the above table).(vii) Write the Nernst equation for this cell only in terms of molality (b), where the mean activity coefficient(y4) of HCl does not feature.(viii) Rearrange the equation in (vii) and make a suitable plot, using the data in the table, to determine thestandard cell potential.Now incorporate the standard cell potential, determined from the linear fit in (vii), into the Nernst(ix)equation and determine the mean activity coefficient (y4) of HCI (and complete the above table).(x)Comment on any differences that you might observe between the values obtained for the meanactivity coefficient (y4) of HCI in (vi) and (ix).

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Consider the following electrochemical cell: Pt|H2(B,p°)|HCI(aq,b)|Hg.Cla(s)| Hg() The potential of this cell, in relation to different molalities (b), has been measured with high precision at 25°C. The following results have been obtained: b/mmol.kg" EN I (ionic strength) Y+ (DHLL) Y+ (linear fit) 1.6077 3.0769 5.0403 7.6938 10.9474 0.60080 0.56825 0.54366 0.52267 0.50532 (i) Write the half-reactions for the cell, and show the standard potential of each half-reaction. (ii) Determine the standard cell potential through simple calculation. (i) Write the cell reaction for this cell.

Consider the following electrochemical cell: Pt|H2(B,p°)|HCI(aq,b)|Hg.Cla(s)| Hg() The potential of this cell, in relation to different molalities (b), has been measured with high precision at 25°C. The following results have been obtained: b/mmol.kg" EN I (ionic strength) Y+ (DHLL) Y+ (linear fit) 1.6077 3.0769 5.0403 7.6938 10.9474 0.60080 0.56825 0.54366 0.52267 0.50532 (i) Write the half-reactions for the cell, and show the standard potential of each half-reaction. (ii) Determine the standard cell potential through simple calculation. (i) Write the cell reaction for this cell.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

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.

Question

Consider the following electrochemical cell:
Pt|H2(g,p°)|HCI(aq,b)|Hg2Cla(s)[ Hg(1)
The potential of this cell, in relation to different molalities (b), has been measured with high precision at
25°C. The following results have been obtained:
b/mmol.kg
E/V
I (ionic strength)
Y: (DHLL)
Y+ (linear fit)
1.6077
3.0769
5.0403
7.6938
10.9474
0.60080
0.56825
0.54366
0.52267
0.50532
(i)
Write the half-reactions for the cell, and show the standard potential of each half-reaction.
(ii)
(ii) Write the cell reaction for this cell.
(iv) Write the Nernst equation for this cell in terms of molality (b) and the mean activity coefficient (ya) of
Determine the standard cell potential through simple calculation.
HCI.
(v) Determine the ionic strength (1) for each molality (b) (and complete the above table).
(vi) By employing the Debye-Hückel limiting law (DHLL), determine the mean activity coefficient (y4) of HCI
(and complete the above table).
(vii) Write the Nernst equation for this cell only in terms of molality (b), where the mean activity coefficient
(y4) of HCl does not feature.
(viii) Rearrange the equation in (vii) and make a suitable plot, using the data in the table, to determine the
standard cell potential.
Now incorporate the standard cell potential, determined from the linear fit in (vii), into the Nernst
(ix)
equation and determine the mean activity coefficient (y4) of HCI (and complete the above table).
(x)
Comment on any differences that you might observe between the values obtained for the mean
activity coefficient (y4) of HCI in (vi) and (ix).

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