Hw many minutes will it take a current of 31.559 Amperes to deposit 1.722 grams of aluminum?

I believe it to be 6.505 minutes

Is this correct? If not, I'll post my work. Thanks

I found 9.757 minutes.

Ok, here's my work, I just plugged in numbers to another problem, I hope this makes sense:

Convert grams to moles:
1.722g x 1g/26.981538mol =.0638214174mol
.0638214174mol x 2 = .1276428349 mol e-
.1276428349 mol e- x 965000 = 12317.53C
t = 12317.53C/ 31.559
t = 6.505

If you don't mind, can you explain where I went wrong. thanks

I tried copying this so I could mark the lines for errors but for some reason I can't copy it. I'll just explain it and you follow along.

#1. You used 2 for the number of electrons. Al is trivalent and the reaction is Al3+ + 3e = Al. That is a major source of your error.

#2. I used 96485 for coulombs in an ampere instead of 96,500. If you are carrying so many decimal places as you show, then you should not round to 96,500; however, this is a minor source of error.

#3. You don't show the conversion to minutes, but I see your work reflects that.

So your 0.12764 will be 0.19146
and that times 96485 = 18,473
and that divided by 31.559 = 585.34 sec and that divided by 60 = 9.76 min.
Check my arithmetic

I didn't obey all the rules for significant figures. You should go through and round the final answer to the right number of s.f. Since 1.722 g has 4 s.f. I think you are allowed 4 in the answer if you use 96,485 and not 96,500.
Also, I forgot to mention that you have one too many zeros on 96500 but that is just a typo since the number doesn't reflect that extra zero.

Yeah I had a lot of errors. Thanks for explaing that.

You're welcome! It's important to be aware of the significant figures and accuracy when performing calculations.

In this case, the main error was using the incorrect number of electrons in the equation. Since aluminum (Al) is trivalent, three electrons are required for the deposition of one mole of aluminum. However, you used two electrons in your calculation. This resulted in an incorrect conversion from moles of aluminum to coulombs.

Additionally, there was a minor error in the conversion factor for coulombs in an ampere. The correct value is 96,485 C/A, not 96,500 C/A. Although this minor error did not have a significant impact on the final answer, it's still important to use the correct conversion factor for accurate calculations.

By correcting these errors and performing the calculation again using the correct number of electrons (0.19146 mol) and conversion factors, we get a result of approximately 9.76 minutes.

Remember to always double-check your calculations, pay attention to significant figures, and use accurate conversion factors for precise results.