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/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
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Transcribed Image Text:3.) Consider that the following half reaction is assigned a half cell voltage of0.00 V.
Hg (aq) + 2 e→ Hg (I)
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/Hg*2.
1.134 V
Sn/Sn2
with
Hg/Hg*2.
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) + 2e → Sn(s)
168
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