1. An example of a nonfaradaic electrochemical process is b. electrodeposition c. adsorption d. passivation 2. Consider a nonfaradaic process showing a constant capacitance per unit area, c, and the relationship q = cE where q is the charge density and E is the electrochemical potential. In cyclic voltammetry, the effect of increasing the potential sweep rate, dEldt (t is time) is to a. corrosion a. increase the current density. b. increase the rate of the corresponding oxidation/reduction process. c. increase the charge transfer resistance. d. all of the above.
1. An example of a nonfaradaic electrochemical process is b. electrodeposition c. adsorption d. passivation 2. Consider a nonfaradaic process showing a constant capacitance per unit area, c, and the relationship q = cE where q is the charge density and E is the electrochemical potential. In cyclic voltammetry, the effect of increasing the potential sweep rate, dEldt (t is time) is to a. corrosion a. increase the current density. b. increase the rate of the corresponding oxidation/reduction process. c. increase the charge transfer resistance. d. all of the above.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Solve 2 please
Transcribed Image Text:1. An example of a nonfaradaic electrochemical process is
b. electrodeposition c. adsorption d. passivation
2. Consider a nonfaradaic process showing a constant capacitance per unit area, c, and the
relationship q = cE where q is the charge density and E is the electrochemical potential. In
cyclic voltammetry, the effect of increasing the potential sweep rate, dEldt (t is time) is to
a. corrosion
a. increase the current density.
b. increase the rate of the corresponding oxidation/reduction process.
c. increase the charge transfer resistance.
d. all of the above.
Expert Solution
Step 1: Electrochemical pprocess
There are two types of electrochemical cells: galvanic, also called Voltaic, and electrolytic. Galvanic cells derives their energy from spontaneous redox reactions, while electrolytic cells involve non-spontaneous reactions and thus require an external electron source like a DC battery or an AC power source.
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