Question

Diamond is one form of elemental carbon engagement ring contains a diamond weighing 1.25 carats (1 carat is equal to 200

mg). ?ow many atoms are present in the Diamond.

Answer 1

1.25 x 10²² carbon atoms

Step-by-step explanation:

The number of atoms in a sample can be calculated using Avogadro's number, which states that 1 mole of a substance contains 6.022 x 10²³ particles. We can use this information to find the number of carbon atoms present in the diamond.

Given that 1 carat is equal to 200 mg, we can convert the weight of the diamond to grams. 1.25 carats is equal to 250 mg, which is equal to 0.25 grams. We can then calculate the number of moles of carbon atoms using the molar mass of carbon (12.01 g/mol).

The number of moles can be calculated using the formula:

moles = mass / molar mass

moles of carbon = 0.25 g / 12.01 g/mol

moles of carbon = 0.02081565412 mol

Finally, we can use Avogadro's number to find the number of atoms:

number of atoms = moles * Avogadro's number

number of atoms = 0.02081565412 mol * 6.022 x 10²³

number of atoms = 1.25 x 10²²

Therefore, there are approximately 1.25 x 10²² carbon atoms present in the diamond.

Answer 2

`1.29x10^(22) atoms`

Step-by-step explanation:

First of all we need to dererminate the diamond mass by transforming carats in grams

`1.25_(carat) *0.200_(g/carat) = 0.250_(g)`

Upon consulting a periodic table one finds the atomic mass of carbon

C=12.01 g/mol

Knowing the carbon mass and the avogrado constant (1 mole =
`6.022x10^(22) atoms`) one compute how many atoms there are in 0.250 g of diamond

`0.250_(g)/12.01_(g/mol)*6.022x10^(22)_(atoms/mol)=1.29x10^(22)_(atoms)`