Chemistry Examples

$N a N O_{3}$

Step 1

To find the mass of $1$ mole of $N a N O_{3}$ 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 $N a N O_{3}$ $=$ $(mass of Na)$ + $(mass of N)$ + $3 (mass of O)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $N a N O_{3}$ $=$ $(22.98999977)$ + $(14.01000022)$ + $3 (16)$

Step 3

Simplify the result.

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Step 3.1

Remove parentheses.

mass of $1$ mole of $N a N O_{3} = 22.98999977 + 14.01000022 + 3 (16) g$

Step 3.2

Multiply $3$ by $16$ .

mass of $1$ mole of $N a N O_{3} = 22.98999977 + 14.01000022 + 48 g$

Step 3.3

Add $22.98999977$ and $14.01000022$ .

mass of $1$ mole of $N a N O_{3} = 37 + 48 g$

Step 3.4

Add $37$ and $48$ .

mass of $1$ mole of $N a N O_{3} = 85 g$

Step 4

Find the mass percentage of $N a$ .

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Step 4.1

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

Mass percentage of $N a = \frac{22.99}{85} \cdot 100$

Step 4.2

Cancel the common factor of $5$ .

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Step 4.2.1

Factor $5$ out of $85$ .

$\frac{22.99}{5 (17)} \cdot 100$

Step 4.2.2

Factor $5$ out of $100$ .

$\frac{22.99}{5 \cdot 17} \cdot (5 \cdot 20)$

Step 4.2.3

Cancel the common factor.

$\frac{22.99}{5 \cdot 17} \cdot (5 \cdot 20)$

Step 4.2.4

Rewrite the expression.

$\frac{22.99}{17} \cdot 20$

Step 4.3

Combine $\frac{22.99}{17}$ and $20$ .

$\frac{22.99 \cdot 20}{17}$

Step 4.4

Simplify the expression.

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Step 4.4.1

Multiply $22.99$ by $20$ .

$\frac{459.8}{17}$

Step 4.4.2

Divide $459.8$ by $17$ .

$27.04705882$

Step 4.5

Set the number as a percent.

Mass percentage of $N a = 27.04705882 %$

Step 5

Find the mass percentage of $N$ .

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Step 5.1

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

Mass percentage of $N = \frac{14.01}{85} \cdot 100$

Step 5.2

Cancel the common factor of $5$ .

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Step 5.2.1

Factor $5$ out of $85$ .

$\frac{14.01}{5 (17)} \cdot 100$

Step 5.2.2

Factor $5$ out of $100$ .

$\frac{14.01}{5 \cdot 17} \cdot (5 \cdot 20)$

Step 5.2.3

Cancel the common factor.

$\frac{14.01}{5 \cdot 17} \cdot (5 \cdot 20)$

Step 5.2.4

Rewrite the expression.

$\frac{14.01}{17} \cdot 20$

Step 5.3

Combine $\frac{14.01}{17}$ and $20$ .

$\frac{14.01 \cdot 20}{17}$

Step 5.4

Simplify the expression.

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Step 5.4.1

Multiply $14.01$ by $20$ .

$\frac{280.2}{17}$

Step 5.4.2

Divide $280.2$ by $17$ .

$16.48235294$

Step 5.5

Set the number as a percent.

Mass percentage of $N = 16.48235294 %$

Step 6

Find the mass percentage of $O$ .

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Step 6.1

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

Mass percentage of $O = \frac{48}{85} \cdot 100$

Step 6.2

Cancel the common factor of $5$ .

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Step 6.2.1

Factor $5$ out of $85$ .

$\frac{48}{5 (17)} \cdot 100$

Step 6.2.2

Factor $5$ out of $100$ .

$\frac{48}{5 \cdot 17} \cdot (5 \cdot 20)$

Step 6.2.3

Cancel the common factor.

$\frac{48}{5 \cdot 17} \cdot (5 \cdot 20)$

Step 6.2.4

Rewrite the expression.

$\frac{48}{17} \cdot 20$

Step 6.3

Combine $\frac{48}{17}$ and $20$ .

$\frac{48 \cdot 20}{17}$

Step 6.4

Multiply $48$ by $20$ .

$\frac{960}{17}$

Step 6.5

Cancel the common factor of $960$ and $17$ .

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Step 6.5.1

Rewrite $960$ as $1 (960)$ .

$\frac{1 (960)}{17}$

Step 6.5.2

Cancel the common factors.

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Step 6.5.2.1

Rewrite $17$ as $1 (17)$ .

$\frac{1 \cdot 960}{1 \cdot 17}$

Step 6.5.2.2

Cancel the common factor.

$\frac{1 \cdot 960}{1 \cdot 17}$

Step 6.5.2.3

Rewrite the expression.

$\frac{960}{17}$

Step 6.6

Set the number as a percent.

Mass percentage of $O = \frac{960}{17 %}$

Step 7

Find the mass percentage of each element in the molecule.

Mass percentage of $N a = 27.04705882 %$

Mass percentage of $N = 16.48235294 %$

Mass percentage of $O = \frac{960}{17 %}$