A voltaic cell consists of an aluminum electrode in a solution of Al(NO3)3 in one beaker, and, in the other beaker, of a platinum electrode immersed in a KCl solution, with Cl2 gas bubbled around it. A salt bridge connects the two aqueous solutions and a metallic wire connects the two electrodes. a) Write the oxidation half-reaction b) Write the reduction half-reaction. c) Write the overall balanced equation d) Which electrode serves as the anode? e) Does the aluminum electrode lose or gain mass as the cell reaction proceed? f) Calculate the standard cell potential Ecell at 25 oC.
A voltaic cell consists of an aluminum electrode in a solution of Al(NO3)3 in one beaker, and, in the other beaker, of a platinum electrode immersed in a KCl solution, with Cl2 gas bubbled around it. A salt bridge connects the two aqueous solutions and a metallic wire connects the two electrodes. a) Write the oxidation half-reaction b) Write the reduction half-reaction. c) Write the overall balanced equation d) Which electrode serves as the anode? e) Does the aluminum electrode lose or gain mass as the cell reaction proceed? f) Calculate the standard cell potential Ecell at 25 oC.
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.43QP: A voltaic cell is constructed from the following half-cells: a chromium electrode in chromium(III)...
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A voltaic cell consists of an aluminum electrode in a solution of Al(NO3)3 in one beaker, and, in the other beaker, of a platinum electrode immersed in a KCl solution, with Cl2 gas bubbled around it. A salt bridge connects the two aqueous solutions and a metallic wire connects the two electrodes.
a) Write the oxidation half-reaction
b) Write the reduction half-reaction.
c) Write the overall balanced equation
d) Which electrode serves as the anode?
e) Does the aluminum electrode lose or gain mass as the cell reaction proceed?
f) Calculate the standard cell potential Ecell at 25 oC.
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