Find the Mass Percentages FeSO_4(7H_2O)

$F e S O_{4} (7 H_{2} O)$

Step 1

To find the mass of $1$ mole of $F e S O_{4} (7 H_{2} O)$ 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 $F e S O_{4} (7 H_{2} O)$ $=$ $(mass of Fe)$ + $(mass of S)$ + $4 (mass of O)$ + $2 (mass of H)$ + $(mass of O)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $F e S O_{4} (7 H_{2} O)$ $=$ $(55.84999847)$ + $(32.06999969)$ + $4 (16)$ + $2 (1.00999999)$ + $(16)$

Step 3

Simplify the result.

Remove parentheses.

mass of $1$ mole of $F e S O_{4} (7 H_{2} O) = 55.84999847 + 32.06999969 + 4 (16) + 2 (1.00999999) + 16 g$

Simplify each term.

Multiply $4$ by $16$ .

mass of $1$ mole of $F e S O_{4} (7 H_{2} O) = 55.84999847 + 32.06999969 + 64 + 2 (1.00999999) + 16 g$

Multiply $2$ by $1.00999999$ .

mass of $1$ mole of $F e S O_{4} (7 H_{2} O) = 55.84999847 + 32.06999969 + 64 + 2.01999998 + 16 g$

Simplify by adding numbers.

Add $55.84999847$ and $32.06999969$ .

mass of $1$ mole of $F e S O_{4} (7 H_{2} O) = 87.91999816 + 64 + 2.01999998 + 16 g$

Add $87.91999816$ and $64$ .

mass of $1$ mole of $F e S O_{4} (7 H_{2} O) = 151.91999816 + 2.01999998 + 16 g$

Add $151.91999816$ and $2.01999998$ .

mass of $1$ mole of $F e S O_{4} (7 H_{2} O) = 153.93999814 + 16 g$

Add $153.93999814$ and $16$ .

mass of $1$ mole of $F e S O_{4} (7 H_{2} O) = 169.93999814 g$

Step 4

Find the mass percentage of $F e$ .

The mass composition percentage is the mass of $F e$ divided by the mass of the entire molecule converted to a percentage.

Mass percentage of $F e = \frac{55.85}{169.93999814} \cdot 100$

Divide $55.85$ by $169.93999814$ .

$0.3286454 \cdot 100$

Multiply $0.3286454$ by $100$ .

$32.86454078$

Set the number as a percent.

Mass percentage of $F e = 32.86454078 %$

Step 5

Find the mass percentage of $S$ .

The mass composition percentage is the mass of $S$ divided by the mass of the entire molecule converted to a percentage.

Mass percentage of $S = \frac{32.07}{169.93999814} \cdot 100$

Divide $32.07$ by $169.93999814$ .

$0.18871366 \cdot 100$

Multiply $0.18871366$ by $100$ .

$18.87136657$

Set the number as a percent.

Mass percentage of $S = 18.87136657 %$

Step 6

Find the mass percentage of $O$ .

The mass composition percentage is the mass of $O$ divided by the mass of the entire molecule converted to a percentage.

Mass percentage of $O = \frac{80}{169.93999814} \cdot 100$

Divide $80$ by $169.93999814$ .

$0.47075438 \cdot 100$

Multiply $0.47075438$ by $100$ .

$47.0754389$

Set the number as a percent.

Mass percentage of $O = 47.0754389 %$

Step 7

Find the mass percentage of $H$ .

The mass composition percentage is the mass of $H$ divided by the mass of the entire molecule converted to a percentage.

Mass percentage of $H = \frac{2.02}{169.93999814} \cdot 100$

Divide $2.02$ by $169.93999814$ .

$0.01188654 \cdot 100$

Multiply $0.01188654$ by $100$ .

$1.18865483$

Set the number as a percent.

Mass percentage of $H = 1.18865483 %$

Step 8

Find the mass percentage of each element in the molecule.

Mass percentage of $F e = 32.86454078 %$

Mass percentage of $S = 18.87136657 %$

Mass percentage of $O = 47.0754389 %$

Mass percentage of $H = 1.18865483 %$

Find the Mass Percentages FeSO_4(7H_2O)

Related Questions

Support LCMGCF.com by disabling your adblocker.