What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Pb²+ concentration is 8.71 x 10-4 M and the Zn²+ concentration is 1.47 M? 2+ Pb²+ (aq) +Zn(s) → Pb(s) + Zn²+ (aq) Pb²+ (aq) + 2e Zn2 n2+ (aq) + 2e → Pb(s) Ee red → Zn(s) Ee red Otrue Ofalse = -0.126 V -0.763 V Ecell = V The cell reaction as written above is spontaneous for the concentrations given:
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Pb²+ concentration is 8.71 x 10-4 M and the Zn²+ concentration is 1.47 M? 2+ Pb²+ (aq) +Zn(s) → Pb(s) + Zn²+ (aq) Pb²+ (aq) + 2e Zn2 n2+ (aq) + 2e → Pb(s) Ee red → Zn(s) Ee red Otrue Ofalse = -0.126 V -0.763 V Ecell = V The cell reaction as written above is spontaneous for the concentrations given:
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2req
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What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the
Pb²+ concentration is
8.71 × 10-4 M and the
Zn2+ concentration is 1.47 M?
#3
E
Pb²+ (aq) + Zn(s) → Pb(s) + Zn²+ (aq)
D
Pb²+ (aq) +2e
Zn2+ (aq) +2e → Zn(s) E
Ecell=1
V
The cell reaction as written above is spontaneous for the concentrations given:
Otrue
Ofalse
Submit Answer
$
4
R
F
07 dº
E
Pb(s) = -0.126 V
red
= -0.763 V
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Transcribed Image Text:eq
2req
[Review Topics]
[References]
Use the References to access important values if needed for this question.
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the
Pb²+ concentration is
8.71 × 10-4 M and the
Zn2+ concentration is 1.47 M?
#3
E
Pb²+ (aq) + Zn(s) → Pb(s) + Zn²+ (aq)
D
Pb²+ (aq) +2e
Zn2+ (aq) +2e → Zn(s) E
Ecell=1
V
The cell reaction as written above is spontaneous for the concentrations given:
Otrue
Ofalse
Submit Answer
$
4
R
F
07 dº
E
Pb(s) = -0.126 V
red
= -0.763 V
→
Retry Entire Group 9 more group attempts remaining
%
5
Cengage Learning Cengage Technical Support
T
G
MacBook Pro
A
6
Y
&
7
H
U
* 00
8
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9
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