Find the Density at STP Li

$L i$

Step 1

To find the mass of $1$ mole of $L i$ 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 $L i$ $=$ $(mass of Li)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $L i$ $=$ $(6.94000005)$

Step 3

Remove parentheses.

mass of $1$ mole of $L i = 6.94000005 g$

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.

$\frac{6.94000005 g}{22.4 L}$

Step 6

Factor $6.94000005$ out of $6.94000005 g$ .

$\frac{6.94000005 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{6.94000005 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{6.94000005}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $6.94000005$ by $22.4$ .

$0.30982143 \frac{g}{L}$

Step 10

Combine $0.30982143$ and $\frac{g}{L}$ .

$\frac{0.30982143 g}{L}$

Find the Density at STP Li

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