Chemistry Examples

$F e_{2} O_{3}$

Step 1

To find the mass of $1$ mole of $F e_{2} O_{3}$ look up the atomic mass of each element and multiply it by the number of atoms contained in each element in the molecule.

Step 2

Fill in the atomic masses from the periodic table.

Step 3

Simplify the result.

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Step 3.1

Simplify each term.

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Step 3.1.1

Multiply $2$ by $55.84999847$ .

mass of $1$ mole of $F e_{2} O_{3} = 111.69999694 + 3 (16) g$

Step 3.1.2

Multiply $3$ by $16$ .

mass of $1$ mole of $F e_{2} O_{3} = 111.69999694 + 48 g$

Step 3.2

Add $111.69999694$ and $48$ .

mass of $1$ mole of $F e_{2} O_{3} = 159.69999694 g$

Step 4

One mole of any gas occupies $22.4 L$ at STP (standard temperature and pressure).

$V = 22.4 L$

Step 5

Density is mass over volume.

$\frac{159.69999694 g}{22.4 L}$

Step 6

Factor $159.69999694$ out of $159.69999694 g$ .

$\frac{159.69999694 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{159.69999694 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{159.69999694}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $159.69999694$ by $22.4$ .

$7.12946414 \frac{g}{L}$

Step 10

Combine $7.12946414$ and $\frac{g}{L}$ .

$\frac{7.12946414 g}{L}$