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posted by  Forensics on 4/25/2008 2:55:50 PM  |  status: Closed  

Electrochemistry

Course Textbook Chapter Problem
General Chemistry N/A N/A N/A
Question Details:
An electrolytic cell is used to plate silver from a silver nitrate solution onto an electrode. How much time (in seconds) is required to deposit 8.0 g of silver if the current is kept constant at 5.0 amperes? Assume 100% current efficiency. (F = 96480 C/mol e-)
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posted by Blackmamba on 4/25/2008 6:37:52 PM  |  status: Live
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"you are a gentleman and a scholar"
Response Details:
1. Write the reaction equation:
Ag+ + e- --> Ag(s)
2. Calculate moles of electrons:
m=8.0 g n=m/M = 8.0g/107.8682gmol-1
moles of Ag = 0.074164 mol
moles of Ag=moles of electrons
3. Calculate time:
n=Q/F , thus Q=nF
Q=(0.074164mol)(96480 C/mol e-) = 7155.7 C
Q=It , thus t=Q/I = 7155.7C/5A = 1413 s

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posted by larios on 4/25/2008 6:44:33 PM  |  status: Live
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