Chemistry Examples

$F e_{2} (S O_{4})$

Step 1

To find the mass of $1$ mole of $F e_{2} (S O_{4})$ 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

Remove parentheses.

mass of $1$ mole of $F e_{2} (S O_{4}) = 2 (55.84999847) + 32.06999969 + 4 (16) g$

Step 3.2

Simplify each term.

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Step 3.2.1

Multiply $2$ by $55.84999847$ .

mass of $1$ mole of $F e_{2} (S O_{4}) = 111.69999694 + 32.06999969 + 4 (16) g$

Step 3.2.2

Multiply $4$ by $16$ .

mass of $1$ mole of $F e_{2} (S O_{4}) = 111.69999694 + 32.06999969 + 64 g$

Step 3.3

Simplify by adding numbers.

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Step 3.3.1

Add $111.69999694$ and $32.06999969$ .

mass of $1$ mole of $F e_{2} (S O_{4}) = 143.76999664 + 64 g$

Step 3.3.2

Add $143.76999664$ and $64$ .

mass of $1$ mole of $F e_{2} (S O_{4}) = 207.76999664 g$

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.

$\frac{207.76999664 g}{22.4 L}$

Step 6

Factor $207.76999664$ out of $207.76999664 g$ .

$\frac{207.76999664 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{207.76999664 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{207.76999664}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $207.76999664$ by $22.4$ .

$9.27544627 \frac{g}{L}$

Step 10

Combine $9.27544627$ and $\frac{g}{L}$ .

$\frac{9.27544627 g}{L}$