Find the Density at STP H_2S

$H_{2} S$

Step 1

To find the mass of $1$ mole of $H_{2} S$ 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 $H_{2} S$ $=$ $2 (mass of H)$ + $(mass of S)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $H_{2} S$ $=$ $2 (1.00999999)$ + $(32.06999969)$

Step 3

Simplify the result.

Remove parentheses.

mass of $1$ mole of $H_{2} S = 2 (1.00999999) + 32.06999969 g$

Multiply $2$ by $1.00999999$ .

mass of $1$ mole of $H_{2} S = 2.01999998 + 32.06999969 g$

Add $2.01999998$ and $32.06999969$ .

mass of $1$ mole of $H_{2} S = 34.08999967 g$

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.

$\frac{34.08999967 g}{22.4 L}$

Step 6

Factor $34.08999967$ out of $34.08999967 g$ .

$\frac{34.08999967 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{34.08999967 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{34.08999967}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $34.08999967$ by $22.4$ .

$1.52187498 \frac{g}{L}$

Step 10

Combine $1.52187498$ and $\frac{g}{L}$ .

$\frac{1.52187498 g}{L}$

Find the Density at STP H_2S

Related Questions