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mariarad [96]
2 years ago
12

Both diamond and graphite (i.e. pencil lead) consist of carbon atoms. They are only different in their crystalline structures. O

ne carat or 0.20 g, of a high-quality diamond costs up to $5000, while 25 g of pencil lead may only cost $2. Determine the numbers of C-atom in diamond vs. graphite which can be obtained with $1.
Chemistry
1 answer:
prisoha [69]2 years ago
6 0

Answer:

Moles of carbon atoms  = 3.33  ×  10^{-6} mol

No. of atoms of C in Diamond  = 2.007 ×   10^{28} atom

Atoms of graphite = 6.27 × 10^{23} Atoms

Explanation:

given data

Cost of 0.2g of diamond = $5000

Cost of 25 g of graphite = $ 2

solution

we know cost of 0.2g of diamond is $ 5000 so that for 1$

if buy 1$ = \frac{0.20}{5000}

1$ = 4.0 × 10^{-5} g Carbon

and Moles of carbon atoms  is express as

Moles of carbon atoms = Given mass of Carbon ÷ atomic mass of C      .........1

Moles of carbon atoms  = 4.0  ×  10^{-5}    g/ 2.0g

Moles of carbon atoms  = 3.33  ×  10^{-6} mol

and

No. of atoms of C in Diamond = No. of moles × Avogadro NO    ..............2

No. of atoms of C in Diamond  = 3.33 ×   10^{-6} mol × 6.022 ×   10^{28}

No. of atoms of C in Diamond  = 2.007 ×   10^{28} atom

Graphite

and wew have given Cost of 25 g of graphite is $2 so for but 1$ we get

for buy $1 = 25÷2  = 12.5 g Of graphite

Moles of graphite = 12.5÷12 = 1.04 mol

Atoms of graphite = 1.04 × 6.022 × 1023

Atoms of graphite = 6.27 × 10^{23} Atoms

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