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Use the Nernst equation to calculate the cell potentials of the following cells at 298 K. (a) 2 Ag*(aq)(0.50 M) + Ni(s) →2 Ag(s) + Ni²*(aq)(0.20 M) (b) Cu(s) + PtCl,?-(aq)(0.10 M) → Cu²*(aq)(0.20 M) +PtCl,?-(aq)(0.10 M) + 2 CI¯(aq)(0.40 M) (c) Pb(s) + SO,²-(aq)(0.30 M) + 2 AgCl(s) → PbSO,(s) + 2 Ag(s) + 2 Cl¯(aq)(0.20 M)

Use the Nernst equation to calculate the cell potentials of the following cells at 298 K. (a) 2 Ag*(aq)(0.50 M) + Ni(s) →2 Ag(s) + Ni²*(aq)(0.20 M) (b) Cu(s) + PtCl,?-(aq)(0.10 M) → Cu²*(aq)(0.20 M) +PtCl,?-(aq)(0.10 M) + 2 CI¯(aq)(0.40 M) (c) Pb(s) + SO,²-(aq)(0.30 M) + 2 AgCl(s) → PbSO,(s) + 2 Ag(s) + 2 Cl¯(aq)(0.20 M)

Principles of Instrumental Analysis
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Chapter22: An Introduction To Electroanalytical Chemistry
Section: Chapter Questions
Problem 22.1QAP: Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 ...
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3. Use the Nernst equation to calculate the cell potentials of the following cells at 298 K. (a) 2 Ag*(aq)(0.50 M) + Ni(s)→2 Ag(s) + Ni²*(aq)(0.20 M) (b) Cu(s) + PtCl,²-(aq)(0.10 M) → Cu²+(aq)(0.20 M) +PtCl,? (aq)(0.10 M) + 2 CI (aq)(0.40 M) (c) Pb(s) + SO,- (aq)(0.30 M) + 2 AgCl(s) – PBSO4(s) + 2 Ag(s) + 2 CI¯(aq)(0.20 M)
Transcribed Image Text:3. Use the Nernst equation to calculate the cell potentials of the following cells at 298 K. (a) 2 Ag*(aq)(0.50 M) + Ni(s)→2 Ag(s) + Ni²*(aq)(0.20 M) (b) Cu(s) + PtCl,²-(aq)(0.10 M) → Cu²+(aq)(0.20 M) +PtCl,? (aq)(0.10 M) + 2 CI (aq)(0.40 M) (c) Pb(s) + SO,- (aq)(0.30 M) + 2 AgCl(s) – PBSO4(s) + 2 Ag(s) + 2 CI¯(aq)(0.20 M)
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