[Violet89]

Using 1.1*10^8, and the fact that one electron has a charge of 1.60*10^-19 coulombs, calculate how many electrons there are in one mole.

I calculated:
1.1*10^8 * (6.022*10^23 / 1.60*10^-19) = 4.14*10^50

Is this correct?

[curiouscat]

Using 1.1*10^8,

What does that mean? 

[Violet89]

Using 1.1*10^8,

What does that mean? 

It is the charge of one mole of electrons that I got from my calculations from my lab experiment.

[Violet89]

Using 1.1*10^8,

What does that mean? 

It is the charge of one mole of electrons that I got from my calculations from my lab experiment.

[curiouscat]

It is the charge of one mole of electrons that I got from my calculations from my lab experiment.

Isn't that ~ the Faraday constant?

F = 96,485.3365(21) C/mol.

You seem way off.

Maybe I don't understand the experiment.

[Violet89]

It is the charge of one mole of electrons that I got from my calculations from my lab experiment.

Isn't that ~ the Faraday constant?

F = 96,485.3365(21) C/mol.

You seem way off.

Maybe I don't understand the experiment.

It is suppose to be, yes. I know it is way off from the Faraday constant. I had to work in a group, and that is what they calculated, so I have to use that number.

I just want to make sure the problem is set up correctly.

[curiouscat]

It is suppose to be, yes. I know it is way off from the Faraday constant. I had to work in a group, and that is what they calculated, so I have to use that number.

OK, even then your method seems wrong. Why do you have "6.022*10^23 " in there?

[Violet89]

It is suppose to be, yes. I know it is way off from the Faraday constant. I had to work in a group, and that is what they calculated, so I have to use that number.

OK, even then your method seems wrong. Why do you have "6.022*10^23 " in there?

It says to use Avogadro's number in my lab book. I am very confused on how I am suppose to solve this problem. 

[fledarmus]

You have to show us your units. Based on the way you've set up your problem, my guess is that somehow in your lab, you obtained the measurement that one mole of electrons had a total charge of 1.1*10^8 coulombs. So your starting measurement is 1.1*10^8 coulombs/mole. Is that right?

Now you are trying to determine the total number of electrons in a mole, using the charge on an electron which is 1.60*10^-19 coulombs/electron.

So as Curiouscat asked, why are you including Avogadro's number, and what units are you attaching to it? The only units that would make sense in context would be electrons/mole, and that is the value you are trying to calculate! All you should need to do is to divide your value for coulombs/mole by your value for coulombs/electron - the coulombs cancel, and you are left with electrons/mole.

So go back to your experiment and attach the units - what value were you actually measuring? 1.1*10^8 what?

[Violet89]

You have to show us your units. Based on the way you've set up your problem, my guess is that somehow in your lab, you obtained the measurement that one mole of electrons had a total charge of 1.1*10^8 coulombs. So your starting measurement is 1.1*10^8 coulombs/mole. Is that right?

Now you are trying to determine the total number of electrons in a mole, using the charge on an electron which is 1.60*10^-19 coulombs/electron.

So as Curiouscat asked, why are you including Avogadro's number, and what units are you attaching to it? The only units that would make sense in context would be electrons/mole, and that is the value you are trying to calculate! All you should need to do is to divide your value for coulombs/mole by your value for coulombs/electron - the coulombs cancel, and you are left with electrons/mole.

So go back to your experiment and attach the units - what value were you actually measuring? 1.1*10^8 what?

Yes, you are correct, 1.1*10^8 coulombs/mole. Thank you very much.

[fledarmus]

So can you carry on from there? How many electrons do you find per mole?