Write the cell notation for an electrochemical cell consisting of an anode where Pb (s) is oxidized to Pb²+ (aq) and a cathode where Cu²+ (aq)is reduced to Cu (s). Assume all aqueous solutions have a concentration of 1 mol/L. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction:(aq) + 2Cu+ (aq) → Pb(s) + 2Cu²+ (aq)AG°Pb²+=Pb²+ (aq) + 2e¯ → Pb(s) Ee = -0.126 Vred2+Cu²+ (aq) + e→ Cu+ (aq) FºredkJK for this reaction would be== 0.153 V+ than one.

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Write the cell notation for an electrochemical cell consisting of an anode where Pb (s) is oxidized to Pb²+ (aq) and a cathode where Cu²+ (aq) is reduced to Cu (s). Assume all aqueous solutions have a concentration of 1 mol/L.

Write the cell notation for an electrochemical cell consisting of an anode where Pb (s) is oxidized to Pb²+ (aq) and a cathode where Cu²+ (aq) is reduced to Cu (s). Assume all aqueous solutions have a concentration of 1 mol/L.

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

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Question

Write the cell notation for an electrochemical cell consisting of an anode where Pb (s) is oxidized to Pb²+ (aq) and a cathode where Cu²+ (aq)
is reduced to Cu (s). Assume all aqueous solutions have a concentration of 1 mol/L.

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction:
(aq) + 2Cu+ (aq) → Pb(s) + 2Cu²+ (aq)
AG°
Pb²+
=
Pb²+ (aq) + 2e¯ → Pb(s) Ee = -0.126 V
red
2+
Cu²+ (aq) + e
→ Cu+ (aq) Fº
red
kJ
K for this reaction would be
=
= 0.153 V
+ than one.

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