How much will #1.2 * 10^46# atoms of carbon weigh?

1 Answer
Nam D.
Mar 30, 2018

#2.4*10^23 \ "g"#

Explanation:

A carbon atom has an average mass of #12.0107 \ "amu"#. Also, one mole of carbon atoms have a mass of #12.0107 \ "g"#.

Recall that one mole of atoms is #6.02*10^23# atoms.

So here, we got:

#(1.2*10^46color(red)cancelcolor(black)"atoms")/(6.02*10^23color(red)cancelcolor(black)"atoms""/mol")~~2*10^22 \ "mol"#

And so, the total mass will be

#2*10^22color(red)cancelcolor(black)"mol"*(12.0107 \ "g")/(color(red)cancelcolor(black)"mol")=2.4*10^23 \ "g"#

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