To find the amount of electrons transferred, we can use Faraday's first law of electrolysis, which states:
"the mass of a substance produced by electrolysis is directly proportional to the quantity of electricity used".
The formula to calculate the amount of electrons transferred is:
n = (q) / (e)
Where:
- n is the amount of electrons transferred
- q is the total charge (current x time)
- e is the elementary charge (1.6 x 10^-19 C)
First, we need to calculate the total charge by multiplying the current by the time:
q = (10.0 A) * (5.00 h)
Next, we need to convert hours to seconds to match the unit of charge (Coulombs):
q = (10.0 A) * (5.00 h) * (3600 s/h)
Now we can substitute the value of q into the formula to find the amount of electrons transferred:
n = [(10.0 A) * (5.00 h) * (3600 s/h)] / (1.6 x 10^-19 C)
Calculating this expression:
n = 1.125 x 10^24 electrons
Therefore, the amount of electrons transferred is approximately 1.125 x 10^24 electrons.
al^3+(l) + 3e = Al(l)
If a current of 10.0 A is applied for 5.00 h to the Hall-Héroult electrolytic cell, then the amount of electrons transferred is
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