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Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. What is Kc for the following balanced reaction, if E° = +.0218v? 32n+2 (aq) + Cr(s) E° = +.0218v 3Zn(s) + 2Cr +3 1.3 x 10-3 2.2 162 .37 (aq)

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. What is Kc for the following balanced reaction, if E° = +.0218v? 32n+2 (aq) + Cr(s) E° = +.0218v 3Zn(s) + 2Cr +3 1.3 x 10-3 2.2 162 .37 (aq)

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Chemistry
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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 29 Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. What is Kc for the following balanced reaction, if E° = +.0218v? 3Zn(s) + 2Cr+3(aq) 1.3 x 10-3 2.2 162 .37 --> 3Zn+2 (aq) + Cr(s) Eº = +.0218v
Transcribed Image Text:QUESTION 29 Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. What is Kc for the following balanced reaction, if E° = +.0218v? 3Zn(s) + 2Cr+3(aq) 1.3 x 10-3 2.2 162 .37 --> 3Zn+2 (aq) + Cr(s) Eº = +.0218v
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