An electrolytic cell produces aluminum from Al2O3 at the rate of ten kilograms a day. Assuming a yield of 100%
a) how many moles of electrons must pass through the cell in one day?
b) how many amperes are passing through the cell?
c) how many moles of oxygen (O2) are being produced simultaneously?
I know I can figure out this problem easily, I'm just really struggling with writing the equation. Can anyone help me with this?
Use unit multipliers:
Start with what you want:
MolesElectrons= 3*molesAluminumatoms
= above* avagnumberatoms/moleAl
or
MolesElectrons=3*10kg/26.98 moles/day
then for amperes, change the above to moles electron per second.
Then convert moles of electrons to ampere (you know the charge on one electron, so you then know the charge/moleElectrons)
For oxygen, write the balanced equation, and use the coefficents to solve.
I don't quite understand how to write the balanced equation for oxygen. I know I have Al2O3 that ends up as Al (is it aluminium ion, or just Al?) and O2 gas, but I don't know what to do with electrons and what not.
Would I have something like this:
Al2O3 --> 2Al + 3/2O2
? But this doesn't seem right because no electrons are included in the equation.
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