Here is a drawing of an electrochemical cell: the reactions that occur in both halves of the cell are: Sn2 + (aq) + 2e- -> Sn (s) E = -0.14 X3 + (aq) + 3e- --> X (s) E =? A. At the close of the circuit, electrons pass and the mass of Sn (s) increases. Mark the anode, cathode, and direction of flow of electrons in the electrical circuit. B. If the standard cell potential is 0.6 volts, what is the redox potential of the half-cell response of X + 3 / X? C. Write the balanced equation for the cell.
Here is a drawing of an electrochemical cell: the reactions that occur in both halves of the cell are: Sn2 + (aq) + 2e- -> Sn (s) E = -0.14 X3 + (aq) + 3e- --> X (s) E =? A. At the close of the circuit, electrons pass and the mass of Sn (s) increases. Mark the anode, cathode, and direction of flow of electrons in the electrical circuit. B. If the standard cell potential is 0.6 volts, what is the redox potential of the half-cell response of X + 3 / X? C. Write the balanced equation for the cell.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 105QAP: Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a)...
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Here is a drawing of an
the reactions that occur in both halves of the cell are:
Sn2 + (aq) + 2e- -> Sn (s) E = -0.14
X3 + (aq) + 3e- --> X (s) E =?
A. At the close of the circuit, electrons pass and the mass of Sn (s) increases. Mark the anode, cathode, and direction of flow of electrons in the electrical circuit.
B. If the standard cell potential is 0.6 volts, what is the redox potential of the half-cell response of X + 3 / X?
C. Write the balanced equation for the cell.
D. Changed the Sn2 + concentrations from 1 M to 0.5M, and the concentrations of X + 3 from 1M to 0.10M calculated the cell potential in this case.
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