Find the Density at STP TiCl_4

$T i C l_{4}$

Step 1

To find the mass of $1$ mole of $T i C l_{4}$ 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 $T i C l_{4}$ $=$ $(mass of Ti)$ + $4 (mass of Cl)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $T i C l_{4}$ $=$ $(47.86999893)$ + $4 (35.45000076)$

Step 3

Simplify the result.

Multiply $4$ by $35.45000076$ .

mass of $1$ mole of $T i C l_{4} = 47.86999893 + 141.80000305 g$

Add $47.86999893$ and $141.80000305$ .

mass of $1$ mole of $T i C l_{4} = 189.67000198 g$

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.

$\frac{189.67000198 g}{22.4 L}$

Step 6

Factor $189.67000198$ out of $189.67000198 g$ .

$\frac{189.67000198 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{189.67000198 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{189.67000198}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $189.67000198$ by $22.4$ .

$8.4674108 \frac{g}{L}$

Step 10

Combine $8.4674108$ and $\frac{g}{L}$ .

$\frac{8.4674108 g}{L}$

Find the Density at STP TiCl_4

Related Questions

Support LCMGCF.com by disabling your adblocker.