Ch.18 - ElectrochemistryWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
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Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
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Ch.4 - Chemical Quantities & Aqueous Reactions
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Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
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Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Gold is electroplated by a current of 0.5 A for a period of 35 minutes from a solution containing the Au3+ ion.  What is the mass of gold deposited on the electrode during this period. (At Wt Au = 197

Solution: Gold is electroplated by a current of 0.5 A for a period of 35 minutes from a solution containing the Au3+ ion.  What is the mass of gold deposited on the electrode during this period. (At Wt Au = 197

Problem

Gold is electroplated by a current of 0.5 A for a period of 35 minutes from a solution containing the Au3+ ion.  What is the mass of gold deposited on the electrode during this period. (At Wt Au = 197 g/mol)

            A)        2.143 g

            B)        0.0119 g

            C)        0.01088 g

            D)        0.715 g

            E)         0.036 g

Solution

We’re being asked to calculate the mass of the gold (Au) deposited on the electrode after 35 minutes. Gold is electroplated from a solution containing Au3+ ion.

Let’s first determine what happens to Au3+:

 Au(s) must be formed from Au3+(aq)
 Au3+ needs to gain 3 e- in order to become Au(s)

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