76v standard electrode potentials 0 ecell 034 v 0 0 0

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Unformatted text preview: || H+ (1 M) | H2 (1 atm) | Pt (s)(+) ° ° ° Ecell = EH + / H − EZn2+ / Zn 2 ° EZn2+ / Zn = −0.76V ° 0.76 = 0 − EZn2+ / Zn ° Zn 2+ (1M ) + 2e- → Zn( s) Ered = −0.76V Standard Electrode Potentials 0 Ecell = 0.34 V 0 0 0 Ecell = Ecathode - Eanode 0 0 0 Ecell = ECu 2+/Cu – EH +/H2 0 0.34 = ECu2+ /Cu - 0 0 ECu 2+ /Cu = 0.34 V (-) Pt (s) | H2 (1 atm) | H+ (1 M) || Cu2+ (1 M) | Cu (s) (+) Anode (oxidation): Cathode (reduction): 2H+ (1 M) + 2e- H2 (1 atm) Cu2+ (1 M) + 2e- H2 (1 atm) + Cu2+ (1 M) Cu (s) Cu (s) + 2H+ (1 M) The more positive E°red , the stronger the oxidizing agent on the left side. The more positive the E°red , the greater the electronpulling power of the reduction half reaction. oxidation state / reduction state oxidizing agent Reduction agent The more negative the E°red, the greater the electrondonating power of the reduction half reaction. The more negative of E°red , negative the stronger the reducing stronger reducing agent on the right side. right Standard reduction Potentials at 25ºC Standard Reduction Potentials Oxidation state Reduction state...
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This document was uploaded on 02/26/2014.

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