Question

A small diamond, which is made of pure carbon, contains too many carbon atoms to count individually. Which is closest to the number of carbon atoms in a 1.0-g diamond?
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A.
3.6 x 10–45 carbon atoms


Student Selected Incorrect
B.
9.2 x 101 carbon atoms


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C.
5.0 x 1022 carbon atoms


Disabled
D.
4,509 carbon atoms

Answer 1

Answer is C, I just answered the question in my Lesson and got it right. Hope it helps :)

Answer 2

Answer:

Answer is option C (5.0 x 10^22 carbon atoms)

Explanation:

To solve this exercise we need to use stoichiometric relations to relate grams of Carbon with atoms of Carbon. These relations are:

a) 1 mol of Carbon atoms = 12 g C (atomic weight of C taken from periodic table)

b) 1 mol of Carbon atomos = 6,022 x 10*23 Carbon atomos (this number is the Avogadros number)

So we will use these two relation to transform grams of Carbon to atoms of Carbon. We will follow this structure:

Unknown variable = Data x "stoichiometric relation 1" x "stoichiometric relation 2"

*Unknown variable = atoms of Carbon

*Data = 1 g of Carbon

*Stoichiometric relation 1 = $\frac{1 mol of Carbon atoms}{12 g of Carbon}$

*Stoichiometric relation 2 = $\frac{6.022 · 10^{23} of Carbon atoms }{1 mol of Carbon}$

Then we will replace information in general structure:

atoms of C =   $1 g of Carbon x$ $\frac{1 mol of Carbon atoms}{12 g of Carbon} x \frac{6.022 ·10^{23} Carbon atoms}{1 mol of Carbon atoms}$

atoms of Carbon = 5,0 x $10^{22}$ atoms of Carbon