How many Cu++ions are deposited on the cathode of copper voltameter if 2.5A current is passed through voltameter for 30 min ?
Answers
5 amperes is 5 coulombs per second, 5C/s
So the total charge in 30 minutes is Q = 5C/s x 30min x 60s/min = 9000C
Then the number of moles of copper plated out (n) is:
n = Q/zF where z is the number of electrons in the half-cell reaction (in this case, 2) and F is the Faraday constant = 96,485/mol
So, n = 9000/(2x96485) = 0.0466mol
And this is 63.546 x 0.0466 = 2.96g
So 2.96 grams are plated deposited at the cathode.
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see.
m=Zit i=5A t=30*60sec
and Z(elctrochemical equivalent)=E/96500 E=63.5/2
m=63.2*5*30*60/96500*2
=1.48gm.
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m=z I t
=. 00033*5*30*60 grams
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