Current is passed through a cell where the half-reaction that occurs at the cathode is 5e + MnO4 + 8H* - Mn2+ + 4H20 All the MnO 4 ions present in 25.0 mL of solution have been reduced after a current of 0.600 ampere has passed for 844 seconds. What was the original concentration of MnO 4 ions? O a. 1.02 x 10-1 M O b.0.21 M О с. 1.47 М O d.7.10 x 10-3 M О е. 420х 10-2 м

Current is passed through a cell where the half-reaction that occurs at the cathode is 5e + MnO4 + 8H* - Mn2+ + 4H20 All the MnO 4 ions present in 25.0 mL of solution have been reduced after a current of 0.600 ampere has passed for 844 seconds. What was the original concentration of MnO 4 ions? O a. 1.02 x 10-1 M O b.0.21 M О с. 1.47 М O d.7.10 x 10-3 M О е. 420х 10-2 м

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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Similar questions

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You want to set up a series of voltaic cells with specific cell potentials. A Zn2+(aq, 1.0 M)| Zn(s) half-cell is in one compartment. Identify several half-cells that you could use so that the cell potential will be close to (a) 1.1 V and (b) 0.50 V. Consider cells in which the zinc cell can be either the cathode or the anode.
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A voltaic cell is constructed using the reaction of chromium metal and iron(II) ions. 2 Cr(s) + 3 Fe2+(aq) 2 Cr3+(aq) + 3 Fe(s) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ________ half-cell to the ______ half-cell. The half-reaction at the anode is _______ and that at the cathode is ________.
Consider the cell Pt|H2|H+H+|H2|Pt In the anode half-cell, hydrogen gas at 1.0 atm is bubbled over a platinum electrode dipping into a solution that has a pH of 7.0. The other half-cell is identical to the first except that the solution around the platinum electrode has a pH of 0.0. What is the cell voltage?
A potential of 0.142 V is recorded (under standard conditions) for a voltaic cell constructed using the following half reactions: Cathode: Pb2+(aq) + 2 e Pb(s) Anode: PbCl2(s) + 2 e Pb(s) + 2 Cl(aq) Net: Pb2+(aq) + 2 Cl(aq) PbCI2(s) (a) What is the standard reduction potential for the anode reaction? (b) Calculate the solubility product, Ksp, for PbCl2.

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