What charge in coulombs is required to deposit 0.301g Cu(s) from a solution of Cu^2+?

Cu^2+ 2e^- = Cu

0.301g/63.5g/mol = 4.7 x 10^-3 mol Cu

(4.7 x 10^-3 mol Cu) (2 mol e^-/mol Cu)

I should be able to mutiply that by 96,500 (Faraday number) to get 914C, but I don't.

Someoneoffered me a number of Coulombs per electron of 1.602x10^-19.

What's the difference between Coulombs per electron and 1 Faraday?

0.301/63.54 x 2 x 96,484 = 914.1 which rounds to 914. Perhaps you're punching the wrong numbers on the calculator.

Well, Coulombs per electron is a measure of the charge carried by a single electron, whereas 1 Faraday is the charge carried by one mole of electrons.

To put it into perspective, if you have a Coulomb per electron, it's like having just one tiny electron helping out with the charge. But if you have 1 Faraday, it's like having a whole mole of electrons lined up, ready to lend a hand with the charge.

You see, a mole of anything is pretty big. It's like a baker's dozen on steroids, except instead of doughnuts, you've got a bunch of electrons. So that's why the Faraday number is so large compared to the charge of a single electron.

In short, Coulombs per electron is like having a solo electron doing its thing, while 1 Faraday is like having a whole elec-troupe ready to perform the charge dance. They may be different, but they're both important in their own electrifying ways!

The difference between Coulombs per electron and 1 Faraday lies in the relationship between charge and the number of electrons involved in a reaction.

1 Faraday (F) is equal to 96,500 Coulombs (C). This value represents the charge required to transfer 1 mole of electrons during an electrochemical reaction.

On the other hand, Coulombs per electron refers to the amount of charge carried by a single electron. The value is approximately 1.602 x 10^-19 Coulombs (C), which represents the fundamental charge of an electron.

To convert between Coulombs and Faradays, you can use the relationship:

1 Faraday (F) = 96,500 Coulombs (C)

So, in your case, if you have the number of moles of electrons involved in the reaction, you can use this conversion factor to calculate the total charge in Coulombs:

Total charge (C) = (Number of moles of electrons) x (1 Faraday)

However, if you have the number of electrons instead of moles of electrons, you can use the charge per electron:

Total charge (C) = (Number of electrons) x (Coulombs per electron)

Coulombs per electron (C/e-) and 1 Faraday (F) are both units of electric charge, but they correspond to different quantities.

Coulombs per electron (C/e-) is a measure of the charge carried by a single electron. The value you were given, 1.602x10^-19 C/e-, represents the charge of one electron in coulombs. This is a fundamental constant and is useful in many calculations involving individual electrons.

On the other hand, 1 Faraday (F) is a much larger unit of electric charge. It is defined as the amount of charge required to deposit one mole of a substance during an electrochemical reaction. The value of 1 Faraday is approximately 96,500 C/mol.

In your case, you correctly determined that 4.7 x 10^-3 mol of Cu is required to deposit 0.301g of Cu. However, to determine the total charge in coulombs, you need to use the Faraday constant (96,500 C/mol) rather than the value of 1.602x10^-19 C/e-.

Here's the correct calculation:

(4.7 x 10^-3 mol Cu) x (2 mol e-/mol Cu) x (96,500 C/mol) = 914C

So, the charge required to deposit 0.301g of Cu from the solution is 914 Coulombs (C).