If you wanted to anodize 1.00 mol of Al to Al₂O3, how many mol of electrons would you need to provide (via the power supply)? The power supplies used in lab have a maximum current rating of 700 mA. Assuming the power supply constantly operated at the maximum current, how long would you need to run the anodization in order to produce 1.00 mol of Al₂O3?
If you wanted to anodize 1.00 mol of Al to Al₂O3, how many mol of electrons would you need to provide (via the power supply)? The power supplies used in lab have a maximum current rating of 700 mA. Assuming the power supply constantly operated at the maximum current, how long would you need to run the anodization in order to produce 1.00 mol of Al₂O3?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:. If you wanted to anodize 1.00 mol of Al to Al2O3, how many mol of electrons would you need to
provide (via the power supply)?
The power supplies used in lab have a maximum current rating of 700 mA. Assuming the power supply
constantly operated at the maximum current, how long would you need to run the anodization in
order to produce 1.00 mol of Al₂O3?
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the answers are diffrernt please can you rechack and see which is correct
Transcribed Image Text:(ay)
I = 700mA = 700 x10³ A = 0.7 A
t = ?
Ammount of A603
2 A1
Now
0₂
+ be©
Aboz = 1 male
> 20173
t=
→ 302
2A+ 202-
* Thus No-of moles of elections per used = 6 moles
(to obtain I mole of A1₂203)
charge required = 6F=6X96500C
Q=Ixt
→→→→> Al2.93
+628
6X96500
6 x765000 sec.
7
t = 13785-7 min
t = 22976 Ans.
6x765.000 min
7 x 60
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