Asked by bernice
calculate the current that must be part into a solution of aluminium salts for 1 hr 30 mins in order to deposit 1.5 gram of aluminium(al=27 if =96500c)
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Use Faraday's law. For Al (valence z = 3):
I = Q / t = (z·F·m / M) / t
where m = 1.5 g, M = 27 g·mol⁻¹, F = 96500 C·mol⁻¹, t = 1.5 h = 5400 s.
n = m/M = 1.5/27 = 0.05556 mol
electrons moles = z·n = 3·0.05556 = 0.16667 mol
Q = 0.16667·96500 = 1.6083×10^4 C
I = Q/t = 1.6083×10^4 / 5400 = 2.98 A
So you need about 3.0 A (assuming 100% current efficiency). If efficiency η < 1, divide this current by η (or multiply by 1/η).
I = Q / t = (z·F·m / M) / t
where m = 1.5 g, M = 27 g·mol⁻¹, F = 96500 C·mol⁻¹, t = 1.5 h = 5400 s.
n = m/M = 1.5/27 = 0.05556 mol
electrons moles = z·n = 3·0.05556 = 0.16667 mol
Q = 0.16667·96500 = 1.6083×10^4 C
I = Q/t = 1.6083×10^4 / 5400 = 2.98 A
So you need about 3.0 A (assuming 100% current efficiency). If efficiency η < 1, divide this current by η (or multiply by 1/η).
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