Find the Density at STP CuCl_2

$C u C l_{2}$

Step 1

To find the mass of $1$ mole of $C u C l_{2}$ 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 $C u C l_{2}$ $=$ $(mass of Cu)$ + $2 (mass of Cl)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $C u C l_{2}$ $=$ $(63.54999923)$ + $2 (35.45000076)$

Step 3

Simplify the result.

Multiply $2$ by $35.45000076$ .

mass of $1$ mole of $C u C l_{2} = 63.54999923 + 70.90000152 g$

Add $63.54999923$ and $70.90000152$ .

mass of $1$ mole of $C u C l_{2} = 134.45000076 g$

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.

$\frac{134.45000076 g}{22.4 L}$

Step 6

Factor $134.45000076$ out of $134.45000076 g$ .

$\frac{134.45000076 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{134.45000076 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{134.45000076}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $134.45000076$ by $22.4$ .

$6.00223217 \frac{g}{L}$

Step 10

Combine $6.00223217$ and $\frac{g}{L}$ .

$\frac{6.00223217 g}{L}$

Find the Density at STP CuCl_2

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