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21. Use the data given below to calculate AG (in kJ/mol) for the following cell reaction at 25 °C: Mg(s) + Sn²*(aq) Mg² (aq) + Sn(s) E° Sn²*/ Sn = -0.14 V E° Mg²/ Mg = -2.37 V [Sn²*] = 1.0 M [Mg²*] = 0.0002 M (R = 8.314 J/mol.K = 0.0821 L.atm/mol.K, Faraday constant = 96500 C/mol.e') * -438 -452 -444 -432 -448

21. Use the data given below to calculate AG (in kJ/mol) for the following cell reaction at 25 °C: Mg(s) + Sn²*(aq) Mg² (aq) + Sn(s) E° Sn²*/ Sn = -0.14 V E° Mg²/ Mg = -2.37 V [Sn²*] = 1.0 M [Mg²*] = 0.0002 M (R = 8.314 J/mol.K = 0.0821 L.atm/mol.K, Faraday constant = 96500 C/mol.e') * -438 -452 -444 -432 -448

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.127QP
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21. Use the data given below to calculate AG (in kJ/mol) for the following cell reaction at 25 °C: Mg(s) + Sn²*(aq) Mg² (aq) + Sn(s) E° Sn²*/ Sn = -0.14 V E° Mg²*/ Mg = -2.37 V [Sn²*] = 1.0 M [Mg²*] = 0.0002 M (R = 8.314 J/mol.K = 0.0821 L.atm/mol.K, Faraday constant = 96500 C/mol.e') * -438 -452 -444 -432 -448
Transcribed Image Text:21. Use the data given below to calculate AG (in kJ/mol) for the following cell reaction at 25 °C: Mg(s) + Sn²*(aq) Mg² (aq) + Sn(s) E° Sn²*/ Sn = -0.14 V E° Mg²*/ Mg = -2.37 V [Sn²*] = 1.0 M [Mg²*] = 0.0002 M (R = 8.314 J/mol.K = 0.0821 L.atm/mol.K, Faraday constant = 96500 C/mol.e') * -438 -452 -444 -432 -448
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