Chemistry Examples

$C H_{3} C H_{2} C {(C H_{3})}_{3}$

Step 1

To find the mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3}$ look up the atomic mass of each element and multiply it by the number of atoms contained in each element in the molecule.

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3}$ $=$ $(mass of C)$ + $3 (mass of H)$ + $(mass of C)$ + $2 (mass of H)$ + $(mass of C)$ + $3 (mass of C)$ + $9 (mass of H)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3}$ $=$ $(12.01000022)$ + $3 (1.00999999)$ + $(12.01000022)$ + $2 (1.00999999)$ + $(12.01000022)$ + $3 (12.01000022)$ + $9 (1.00999999)$

Step 3

Simplify the result.

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Step 3.1

Remove parentheses.

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = (12.01000022) + 3 (1.00999999) + 12.01000022 + 2 (1.00999999) + 12.01000022 + 3 (12.01000022) + 9 (1.00999999) g$

Step 3.2

Simplify each term.

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Step 3.2.1

Multiply $3$ by $1.00999999$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 12.01000022 + 3.02999997 + 12.01000022 + 2 (1.00999999) + 12.01000022 + 3 (12.01000022) + 9 (1.00999999) g$

Step 3.2.2

Multiply $2$ by $1.00999999$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 12.01000022 + 3.02999997 + 12.01000022 + 2.01999998 + 12.01000022 + 3 (12.01000022) + 9 (1.00999999) g$

Step 3.2.3

Multiply $3$ by $12.01000022$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 12.01000022 + 3.02999997 + 12.01000022 + 2.01999998 + 12.01000022 + 36.03000068 + 9 (1.00999999) g$

Step 3.2.4

Multiply $9$ by $1.00999999$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 12.01000022 + 3.02999997 + 12.01000022 + 2.01999998 + 12.01000022 + 36.03000068 + 9.08999991 g$

Step 3.3

Simplify by adding numbers.

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Step 3.3.1

Add $12.01000022$ and $3.02999997$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 15.0400002 + 12.01000022 + 2.01999998 + 12.01000022 + 36.03000068 + 9.08999991 g$

Step 3.3.2

Add $15.0400002$ and $12.01000022$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 27.05000042 + 2.01999998 + 12.01000022 + 36.03000068 + 9.08999991 g$

Step 3.3.3

Add $27.05000042$ and $2.01999998$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 29.07000041 + 12.01000022 + 36.03000068 + 9.08999991 g$

Step 3.3.4

Add $29.07000041$ and $12.01000022$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 41.08000063 + 36.03000068 + 9.08999991 g$

Step 3.3.5

Add $41.08000063$ and $36.03000068$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 77.11000132 + 9.08999991 g$

Step 3.3.6

Add $77.11000132$ and $9.08999991$ .

mass of $1$ mole of $C H_{3} C H_{2} C {(C H_{3})}_{3} = 86.20000123 g$

Step 4

Find the mass percentage of $C$ .

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Step 4.1

The mass composition percentage is the mass of $C$ divided by the mass of the entire molecule converted to a percentage.

Mass percentage of $C = \frac{72.06}{86.20000123} \cdot 100$

Step 4.2

Divide $72.06$ by $86.20000123$ .

$0.83596286 \cdot 100$

Step 4.3

Multiply $0.83596286$ by $100$ .

$83.5962865$

Step 4.4

Set the number as a percent.

Mass percentage of $C = 83.5962865 %$

Step 5

Find the mass percentage of $H$ .

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Step 5.1

The mass composition percentage is the mass of $H$ divided by the mass of the entire molecule converted to a percentage.

Mass percentage of $H = \frac{14.14}{86.20000123} \cdot 100$

Step 5.2

Divide $14.14$ by $86.20000123$ .

$0.16403712 \cdot 100$

Step 5.3

Multiply $0.16403712$ by $100$ .

$16.40371206$

Step 5.4

Set the number as a percent.

Mass percentage of $H = 16.40371206 %$

Step 6

Find the mass percentage of each element in the molecule.

Mass percentage of $C = 83.5962865 %$

Mass percentage of $H = 16.40371206 %$