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A solution containing 0.18 M Pb2+, 1.5 x 10-6 M Pb++, 1.5 x 10-6 M Mn²+ , 0.18 M Mno, , and 0.81 M HNO, was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur. 5 [Pb+ + 2e- = Pb2+] 2 [MnO, + 8H* +5e = Mn²+ + 4H,0] 5 Pb+ + 2 Mn2+ + 8 H,0=5Pb2+ + 2 MnO, + 16H* E: = 1.690 V E = 1.507 V Determine Eu, AG“, and K for this reaction. Esell 3.197 V AG = -3085.105 J K = Calculate the value for the cell potential, Ecell, and the free energy, AG, for the given conditions. Ecell = V AG = J Calculate the value of Ecell for this system at equilibrium. Ecell = V Determine the pH at which the given concentrations of Pb2+, Pb, Mn²+, and MnO, would be at equilibrium. pH = 0.27

A solution containing 0.18 M Pb2+, 1.5 x 10-6 M Pb++, 1.5 x 10-6 M Mn²+ , 0.18 M Mno, , and 0.81 M HNO, was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur. 5 [Pb+ + 2e- = Pb2+] 2 [MnO, + 8H* +5e = Mn²+ + 4H,0] 5 Pb+ + 2 Mn2+ + 8 H,0=5Pb2+ + 2 MnO, + 16H* E: = 1.690 V E = 1.507 V Determine Eu, AG“, and K for this reaction. Esell 3.197 V AG = -3085.105 J K = Calculate the value for the cell potential, Ecell, and the free energy, AG, for the given conditions. Ecell = V AG = J Calculate the value of Ecell for this system at equilibrium. Ecell = V Determine the pH at which the given concentrations of Pb2+, Pb, Mn²+, and MnO, would be at equilibrium. pH = 0.27

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter20: Chemistry Of The Metals
Section: Chapter Questions
Problem 39QAP: Iron(II) can be oxidized to iron(III) by permanganate ion in acidic solution. The permanganate ion...
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A solution containing 0.18 M Pb2+, 1.5 × 10-6 M Pb+, 1.5 x 10-6 M Mn2+, 0.18 M MnO,, and 0.81 M HNO, was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur. 5 [Pb4+ + 2e- = Pb2+] 2 [MnO, + 8 H+ + 5e¯ 2 Mn²+ + 4 H,O] 5 Pb4+ + 2 Mn²+ + 8 H,0 =5 Pb²+ + 2 MnO + 16 H* E; = 1.690 V E` = 1.507 V Determine Eu: AG", and K for this reaction. 3.197 V AG = -3085.105 K = Calculate the value for the cell potential, Ecell, and the free energy, AG, for the given conditions. Ecell = V AG = Calculate the value of Ecell for this system at equilibrium. Ecell = Determine the pH at which the given concentrations of Pb2+, Pb4+ , Mn²+ , and MnO, would be at equilibrium. pH = 0.27
Transcribed Image Text:A solution containing 0.18 M Pb2+, 1.5 × 10-6 M Pb+, 1.5 x 10-6 M Mn2+, 0.18 M MnO,, and 0.81 M HNO, was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur. 5 [Pb4+ + 2e- = Pb2+] 2 [MnO, + 8 H+ + 5e¯ 2 Mn²+ + 4 H,O] 5 Pb4+ + 2 Mn²+ + 8 H,0 =5 Pb²+ + 2 MnO + 16 H* E; = 1.690 V E` = 1.507 V Determine Eu: AG", and K for this reaction. 3.197 V AG = -3085.105 K = Calculate the value for the cell potential, Ecell, and the free energy, AG, for the given conditions. Ecell = V AG = Calculate the value of Ecell for this system at equilibrium. Ecell = Determine the pH at which the given concentrations of Pb2+, Pb4+ , Mn²+ , and MnO, would be at equilibrium. pH = 0.27
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