Find the Density at STP SgSiBH

$S g S i B H$

Step 1

To find the mass of $1$ mole of $S g S i B H$ 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 $S g S i B H$ $=$ $(mass of Sg)$ + $(mass of Si)$ + $(mass of B)$ + $(mass of H)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $S g S i B H$ $=$ $(266)$ + $(28.09000015)$ + $(10.81000041)$ + $(1.00999999)$

Step 3

Simplify the result.

Remove parentheses.

mass of $1$ mole of $S g S i B H = 266 + 28.09000015 + 10.81000041 + 1.00999999 g$

Add $266$ and $28.09000015$ .

mass of $1$ mole of $S g S i B H = 294.09000015 + 10.81000041 + 1.00999999 g$

Add $294.09000015$ and $10.81000041$ .

mass of $1$ mole of $S g S i B H = 304.90000057 + 1.00999999 g$

Add $304.90000057$ and $1.00999999$ .

mass of $1$ mole of $S g S i B H = 305.91000056 g$

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.

$\frac{305.91000056 g}{22.4 L}$

Step 6

Factor $305.91000056$ out of $305.91000056 g$ .

$\frac{305.91000056 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{305.91000056 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{305.91000056}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $305.91000056$ by $22.4$ .

$13.65669645 \frac{g}{L}$

Step 10

Combine $13.65669645$ and $\frac{g}{L}$ .

$\frac{13.65669645 g}{L}$

Find the Density at STP SgSiBH

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