Mole help  [ENDORSED]

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RBergtraun_3A
Posts: 41
Joined: Wed Feb 20, 2019 12:15 am

Mole help

Postby RBergtraun_3A » Sat Oct 05, 2019 4:39 pm

Hi guys! Can anyone explain moles to me in a simple way? I get what they are technically, but it's still not completely clear in my mind. Thanks

Rhea Shah 2F
Posts: 97
Joined: Thu Jul 25, 2019 12:17 am

Re: Mole help

Postby Rhea Shah 2F » Sat Oct 05, 2019 4:55 pm

A mole is a unit of measurement that tells you how much of that element is needed to have 6.02 x 10^23 atoms of that element. The molar mass of each element that is listed on the periodic table is the amount in grams of that element needed to obtain that certain amount of atoms.

kevinchang_4I
Posts: 55
Joined: Tue Nov 13, 2018 12:17 am

Re: Mole help

Postby kevinchang_4I » Sat Oct 05, 2019 4:56 pm

So 1 mol is equal to 6.02 x 10^23 atoms of whatever element you have. It is a standard unit used to simplify and streamline calculations. (Even if it doesn't seem so helpful now) For example, one mol of Carbon is 6.02 x 10^23 individual atoms of Carbon. Now we combine this with the molar mass of Carbon which is around 12 grams/mol, which is also the same as saying 6.02 x 10^23 atoms of Carbon will weigh about 12 grams. Hope this helps!

Aarja Pavade 1H
Posts: 103
Joined: Sat Aug 17, 2019 12:18 am

Re: Mole help

Postby Aarja Pavade 1H » Sun Oct 06, 2019 2:08 pm

Also, keep in mind that in chemistry, atoms are not created or destroyed. As mentioned before, since moles refer to the number of atoms, moles of solute will always remain the somewhen diluting a solution.

Kimme Chun 1I
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Re: Mole help  [ENDORSED]

Postby Kimme Chun 1I » Sun Oct 06, 2019 3:08 pm

A mole is a unit of measurement similar to a dozen. When you say you have a dozen of something, you have 12 of it. When you say you have a mole of something, it means there are 6.022*10^23 of it

gferg21
Posts: 51
Joined: Sat Aug 17, 2019 12:17 am

Re: Mole help

Postby gferg21 » Sun Oct 06, 2019 3:51 pm

When you look on the periodic table and see the mass of one carbon mole (12.011g) or another element, the number just means essentially how much mass a mole of that element is. One mole of carbon by itself is 12.011 grams, for example. it is just a simplified unit of measurement.

Bryce Barbee
Posts: 103
Joined: Wed Sep 18, 2019 12:20 am

Re: Mole help

Postby Bryce Barbee » Sun Oct 06, 2019 4:05 pm

I find it easy to think of moles when I think of them in something other than a chemistry example. When I think about them as strictly just being a unit of measurement for anything, such as fruit, then the idea becomes simpler.

Victoria Otuya 4F
Posts: 50
Joined: Wed Sep 18, 2019 12:21 am

Re: Mole help

Postby Victoria Otuya 4F » Wed Oct 09, 2019 12:43 am

Is it true that when you want to change mass to moles, you use the conversion: mass multiply by 1 mole and divide by the total atomic mass of the element?

Benjamin Feng 1B
Posts: 102
Joined: Sat Sep 07, 2019 12:19 am

Re: Mole help

Postby Benjamin Feng 1B » Wed Oct 09, 2019 12:46 am

Yes that's right. You can check if you're doing the right thing by writing out the dimensional analysis. Start with grams and multiply by mols/gram. Just like multiplying fractions, the grams in both cancel out and you are left with moles. To convert from moles to grams, you would instead multiply by grams/mol.


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