Chemistry 12th Edition

Published by McGraw-Hill Education
ISBN 10: 0078021510
ISBN 13: 978-0-07802-151-0

Chapter 3 - Mass Relationships in Chemical Reactions - Questions & Problems - Page 113: 3.110


$2.4\times10^{24}$ carbon atoms

Work Step by Step

Start by converting 200mg to g by dividing by 1000. $200$ mg$\div1000=0.2$ g The diamond is 24 carats, so multiply 0.2 by 24 to find how many grams total of carbon there are. $0.2$ g$\times24=4.8$ g The molar mass of carbon is 12.011 g/mol. Convert 4.8 g to moles. $\frac{4.8 g}{1}\times\frac{1mol}{12.011g}\approx0.4mol$ One mole of something equals $6.022\times10^{23}$ individual things. So, multiply the amount of moles by $6.022\times10^{23}$ to get the number of atoms: $0.4mol\times(6.022\times10^{23})=2.4\times10^{24}$ atoms
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