What would be the mass of #4.5xx10^26# carbon atoms?

2 Answers
May 18, 2017

Answer:

Well, the mass of #6.022xx10^23# carbon atoms is #12.011*g#.

Explanation:

How do we know this? Well, #6.022xx10^23# individual #""^12C# atoms has a mass of #12.00*g# precisely, and we use this number as a bridge between the sub-micro world of atoms and molecules to the macro world of grams, and litres, that which we can quantitatively measure.

And so.........

#"Mass of carbon"=(4.5xx10^26*"carbon atoms"xx12.011*g)/(6.022xx10^23*"carbon atoms")#

#~=9*kg# carbon...........

May 18, 2017

Answer:

We will convert to mols.

Explanation:

1 mol of #C# has 6.02xx10^23 atoms (Avogadro's number).

So the number you mention contains:

#(4.5xx10^26)/(6.02xx10^23)=0.748xx10^3mol#

Since 1 mol of #C# has a mass of #12.01g#

Total mass #=12.01xx0.748xx10^3=8.98xx10^3g~~9.0kg#