A spoon was silver-plated electrolytically in a AgNO3 solution. If 0.750 g of Ag was deposited on the spoon at a constant current of 20.0 mA, how long (in hours) did the electrolysis take? (1 mA = 1x10–3 A)
11.9 hr
9.32 hr
5.92 hr
8.76 hr
10.1 hr
Answer
9.32 hr
Explanation
Ag+(aq) + e -------> Ag(s)
1mole of electrons is required to deposite 1mole of Ag+
Number of moles of Ag+ = 0.750g /107.87g/mol = 0.006953mol
number of moles of electrons required = 0.006953mol
Number of Columbs required = 0.006953mol × 96485C/mol = 670.86C
20.0mA = 0.0200A
1Ambs = 1Coloumb per second
0.0200A = 0.0200Couloumbs per second
Therefore
Time required for electrolysis = 670.86C/0.0200C/s = 33543s = 9.32 hr
A spoon was silver-plated electrolytically in a AgNO3 solution. If 0.750 g of Ag was deposited...
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