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31. Given the standard reduction potential (E0) values below, calculate the equilibrium constant (Keq) for the reaction: 2 Sn(OH)² (aq) + Si(s) — ->2 HSnO₂ (aq) + SiO² (aq) + 5 H₂O Sn² +2e + Sn²+ E +0.15V Si+ 4e + Si4- E=-1.37V (Assume that this reaction happens in a weakly acidic solution.) =

31. Given the standard reduction potential (E0) values below, calculate the equilibrium constant (Keq) for the reaction: 2 Sn(OH)² (aq) + Si(s) — ->2 HSnO₂ (aq) + SiO² (aq) + 5 H₂O Sn² +2e + Sn²+ E +0.15V Si+ 4e + Si4- E=-1.37V (Assume that this reaction happens in a weakly acidic solution.) =

Chemistry
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
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 88E: For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1,...
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31. Given the standard reduction potential (E0) values below, calculate the equilibrium constant (Keq) for the reaction: 2 Sn(OH)6²(aq) + Si(s)->2 HSnO2 (aq) + SiO3- (aq) +5 H₂O Sn² +2e Sn²+ E°= +0.15V Si + 4e Si4- E=-1.37V (Assume that this reaction happens in a weakly acidic solution.) -
Transcribed Image Text:31. Given the standard reduction potential (E0) values below, calculate the equilibrium constant (Keq) for the reaction: 2 Sn(OH)6²(aq) + Si(s)->2 HSnO2 (aq) + SiO3- (aq) +5 H₂O Sn² +2e Sn²+ E°= +0.15V Si + 4e Si4- E=-1.37V (Assume that this reaction happens in a weakly acidic solution.) -
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