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
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I am not sure if the answers I have entered are correct, I am just very stuck. All info I have is in the pictures above.
![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8d4ce504-fd1c-46df-8d29-413ae89266e8%2F0545395e-e2b0-44a7-ada8-0082b537670b%2Fq96i4re_processed.jpeg&w=3840&q=75)
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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