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When the Pb²+ concentration is 1.41 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.156v. What is the Mn² concentration? Pb2 (aq) Mn(s) Pb(s) + Mn²(aq) Answer: M

When the Pb²+ concentration is 1.41 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.156v. What is the Mn² concentration? Pb2 (aq) Mn(s) Pb(s) + Mn²(aq) Answer: M

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
Chapter1: Chemical Foundations
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When the Pb²+ concentration is 1.41 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.156v. What is the Mn²* concentration? Pb2 (aq) Mn(s) Pb(s) + Mn²(aq) Answer: M
Transcribed Image Text:When the Pb²+ concentration is 1.41 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.156v. What is the Mn²* concentration? Pb2 (aq) Mn(s) Pb(s) + Mn²(aq) Answer: M
The following standard reduction potentials have been determined for the aqueous chemistry of manganese: Mn3+ (aq) + eMn²+ (aq) Mn2+ (aq) + 2e →→→→Mn(s) E° = 1.510 V Eº = -1.029 V Calculate the equilibrium constant (K) for the disproportionation of Mn2*(aq) at 25 °C. 3Mn2+ (aq) = Mn(s) + 2Mn³+ (aq) K =
Transcribed Image Text:The following standard reduction potentials have been determined for the aqueous chemistry of manganese: Mn3+ (aq) + eMn²+ (aq) Mn2+ (aq) + 2e →→→→Mn(s) E° = 1.510 V Eº = -1.029 V Calculate the equilibrium constant (K) for the disproportionation of Mn2*(aq) at 25 °C. 3Mn2+ (aq) = Mn(s) + 2Mn³+ (aq) K =
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