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VMariaS [17]
2 years ago
7

If you have 100.0 grams of carbon and 100.0 grams or iron, which sample will contain more atoms

Chemistry
1 answer:
vodomira [7]2 years ago
6 0
First you need to solve for the number of moles in each. 
1 mole of anything = atomic mas of that element (g)

Carbon has an atomic mass of 12.0107
1 mole of Carbon = 12.0107 g

Iron has an atomic mass of 55.845
1 mole of Iron = 55.845 g

now convert each from grams to moles 
(grams of Carbon cancel and you are left with moles of carbon)
<u>100.0 g Carbon x 1 mol Carbon </u> = 8.326 mol Carbon
       12.0107 g Carbon

(grams of Iron will cancel and you are left with moles of iron)
<u>100.0 g Iron x 1 mol Iron</u> = 1.791 mol Iron
      55.845 g Iron

now we can use avogadro's number to solve for the amount of atoms in each 
1 mol = 6.02x10^23 atoms

<u>8.326 mol Carbonx 6.02 x 10^23 atoms </u> = 5.012 x 10^24 atoms Carbon<u>
</u>        1 mol Carbon
<u>
</u><u>1.791 mol Iron x 6.02 x 10^23 atoms </u> = 1.078 x 10^24 atoms Iron<u>
</u>        1 mol Iron
<u>
</u>5.012 x 10^24 atoms Carbon > 1.078 x 10^24 atoms Iron
<u>
</u>
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Answer:

0.22

Explanation:

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The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

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Given, Mass of C_{2}H_{5}OH = 125.5 g

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The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

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4 0
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Explanation:

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