Find the Density at STP H_2SO_4

$H_{2} S O_{4}$

Step 1

To find the mass of $1$ mole of $H_{2} S O_{4}$ 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 $H_{2} S O_{4}$ $=$ $2 (mass of H)$ + $(mass of S)$ + $4 (mass of O)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $H_{2} S O_{4}$ $=$ $2 (1.00999999)$ + $(32.06999969)$ + $4 (16)$

Step 3

Simplify the result.

Remove parentheses.

mass of $1$ mole of $H_{2} S O_{4} = 2 (1.00999999) + 32.06999969 + 4 (16) g$

Simplify each term.

Multiply $2$ by $1.00999999$ .

mass of $1$ mole of $H_{2} S O_{4} = 2.01999998 + 32.06999969 + 4 (16) g$

Multiply $4$ by $16$ .

mass of $1$ mole of $H_{2} S O_{4} = 2.01999998 + 32.06999969 + 64 g$

Simplify by adding numbers.

Add $2.01999998$ and $32.06999969$ .

mass of $1$ mole of $H_{2} S O_{4} = 34.08999967 + 64 g$

Add $34.08999967$ and $64$ .

mass of $1$ mole of $H_{2} S O_{4} = 98.08999967 g$

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.

$\frac{98.08999967 g}{22.4 L}$

Step 6

Factor $98.08999967$ out of $98.08999967 g$ .

$\frac{98.08999967 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{98.08999967 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{98.08999967}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $98.08999967$ by $22.4$ .

$4.37901784 \frac{g}{L}$

Step 10

Combine $4.37901784$ and $\frac{g}{L}$ .

$\frac{4.37901784 g}{L}$

Find the Density at STP H_2SO_4

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