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)
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
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