[stdaad]

I just want to verify that I am getting this stuff correct. I know its simple but my brain has just stopped working.

I am give the following info about Carbon

Mass of one atom ( I got 12.01 AMU?? )

Mass of one mole ( I got 12.01 g?? )

Number of atoms in one mole ( I think this has something to do with Avogadro's number but I don't know how to figure is out. Would it be:

12.01g X 6.022 x 10(superscript 23)
1G

[Perito]

I just want to verify that I am getting this stuff correct. I know it's simple but my brain has just stopped working.

I hope your brain hasn't stopped working. If it had, you might not know it, but everyone else would. :rolleyes:

Mass of one atom ( I got 12.01 AMU?? )
Mass of one mole ( I got 12.01 g?? )

Looks OK to me. If you wanted more significant figures, it's 12.0107.

Number of atoms in one mole ( I think this has something to do with Avogadro's number but I don't know how to figure is out. Would it be:

Close, but not quite. The 12.01 g shouldn't be in there.

You're correct about Avogadro's number. One mole of any substance contains Avogadro's number of particles. Let me give you an example. (Carbon isn't the best example).

If you have one mole of water, , you have molecules of water. Since there are three atoms per molecule of water (two hydrogen atoms and one oxygen atom), there are atoms in that particular mole.

We normally consider that there is one atom per molecule of carbon. I won't get into the complexities of this (Carbon - Wikipedia, the free encyclopedia). If that be true, then there are Avogadro's number of atoms in one mole of carbon. If you said that carbon was , for example, there would be 20 times Avogadro's number of atoms in that mole.

[stdaad]

Thank You!! When I looked at the question that was my first thought but it seemed to easy an answer. So, I thought some more on it. OOPS! Teach me to think too hard. Again, thank you.