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?

Disabled
A.
3.6 x 10–45 carbon atoms


Student Selected Incorrect
B.
9.2 x 101 carbon atoms


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

Step-by-step 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 =
`(1 mol of Carbon atoms)/(12 g of Carbon)`

*Stoichiometric relation 2 =
`(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`
`(1 mol of Carbon atoms)/(12 g of Carbon) x (6.022 ·10^(23) Carbon atoms)/(1 mol of Carbon atoms)`

atoms of Carbon = 5,0 x
`10^(22)` atoms of Carbon