Find the Density at STP C

$C$

Step 1

To find the mass of $1$ mole of $C$ 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 $C$ $=$ $(mass of C)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $C$ $=$ $(12.01000022)$

Step 3

Remove parentheses.

mass of $1$ mole of $C = 12.01000022 g$

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.

$\frac{12.01000022 g}{22.4 L}$

Step 6

Factor $12.01000022$ out of $12.01000022 g$ .

$\frac{12.01000022 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{12.01000022 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{12.01000022}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $12.01000022$ by $22.4$ .

$0.53616072 \frac{g}{L}$

Step 10

Combine $0.53616072$ and $\frac{g}{L}$ .

$\frac{0.53616072 g}{L}$

Find the Density at STP C

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