Electrolysis calculations?
2018-05-09 11:59 pm
20 amperes of electrode current is passed through molten Al2O3 for two hours. How many moles of electrons are passed through the molten Al2O3?
回答 (2)
2018-05-10 12:25 am
Amount of electricity = I t = (20 A) × (2 × 3600 s) = 144000 C
Each mole of electrons carries 96485 C of electricity.
No. of moles of electrons = (144000 C) / (96485 C/mol) = 1.49 mol
Each mole of electrons carries 96485 C of electricity.
No. of moles of electrons = (144000 C) / (96485 C/mol) = 1.49 mol
2018-05-10 1:11 am
Electrolysis....
Current is a measure of the flow of charge, and is measured in coulomb's second, and given by the derived units of amperes.
1 ampere = 1 coulomb / 1 sec
The "Faraday" is a measure of charge. It is the charge on 1 mole of electrons.
1 F = 6.022x10^23 e- x (1.602x10^-19 C / 1 e-) = 96472 C
2 hrs x (3600 s / 1hr) x (20.0 C / s) x (1 mol e- / 96472 C) = 1.49 mol e- ............. expressed to an "average" three significant digits. A time of "two hours" carries no implication of precision.
Current is a measure of the flow of charge, and is measured in coulomb's second, and given by the derived units of amperes.
1 ampere = 1 coulomb / 1 sec
The "Faraday" is a measure of charge. It is the charge on 1 mole of electrons.
1 F = 6.022x10^23 e- x (1.602x10^-19 C / 1 e-) = 96472 C
2 hrs x (3600 s / 1hr) x (20.0 C / s) x (1 mol e- / 96472 C) = 1.49 mol e- ............. expressed to an "average" three significant digits. A time of "two hours" carries no implication of precision.
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