1) Determine moles of Ag plated out:
1 g divided by 26.98 g/mole = 0.037064 mol
2) Determine moles of electrons required:
Ag+ + 1e¯ ---> Ag
therefore, every mole of Ag plated out requires one mol of electrons.
0.037064 mol x 2 = 0.074128 mol e¯ required
3) Convert moles of electrons to Coulombs of charge:
0.074128 mol e¯ x 96,485.309 C/mol (Faraday constant) = 7152.3579 C
4) Convert to seconds required to deliver the Coulombs determined in step 3 (remember that 1 A = 1 C/sec):
7152.3579 C divided by 2 C/sec = 3576.1789 sec
5) Convert to hours:
3576.1789 sec divided by 3600 sec/hour = 0.9933 hours (Can round up to 1 hour)
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