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 9.40 x 10-4 M and the Zn²+ concentration is 1.18 M? Pb²+ (aq) + Zn(s) → Pb(s) + Zn²+ (aq) Pb²+ (aq) + 2e → Pb(s) Ee red Ecell = -0.126 V Zn²+ (aq) + 2e¯¯ → Zn(s) E -0.763 V red V O true Ofalse B 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 9.40 x 10-4 M and the Zn²+ concentration is 1.18 M? Pb²+ (aq) + Zn(s) → Pb(s) + Zn²+ (aq) Pb²+ (aq) + 2e → Pb(s) Ee red Ecell = -0.126 V Zn²+ (aq) + 2e¯¯ → Zn(s) E -0.763 V red V O true Ofalse B The cell reaction as written above is spontaneous for the concentrations given:
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.152QP
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Transcribed Image Text: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 9.40 x 10-4 M and the Zn² concentration is 1.18 M?
2+
Pb²+ (aq) + Zn(s) → Pb(s) + Zn²+ (aq)
Pb²+ (aq) + 2e¯¯ → Pb(s) Ere
red
2+
Zn²+ (aq) + 2e → Zn(s) E
red
=
Ecell
The cell reaction as written above is spontaneous for the concentrations
given:
-0.126 V
-0.763 V
O true
O false
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