AAMC FL #7 Question 51

[lamborghiniMD]

---

Members do not see this ad.

Approximately how many moles of Al3+ are reduced when .1 faraday of charge passes through a cell during the production of Al? Assume Al3+ is reduced to Al metal only.

The answer is .033mol, but can anyone show me how you would solve this? I had no idea. I have the paper version so I don't have explanations to answers for this test. Thanks!

 

[msamp]

if you need the explanations pm me with your email address

 

[sciencebooks]

if you need the explanations pm me with your email address

👍 Sorry, I love seeing friendly people. Unfortunately, I've noticed way too many cut throat pre-meds in person.

 

[sciencebooks]

OP, I can also give an explanation here if need? 🙂

 

[msamp]

A faraday is equal to the charge found in one mole of electrons. Given a value expressed in faradays and a reduction half reaction, we have to calculate the number of moles being used up.

Al3+ + 3e– → Al

Based on the half reaction, we know that three electrons are used up for every mole of Al3+ that gets reduced. Next, we can use dimensional analysis to calculate the number of moles of Al3+: