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## PowerPoint Slideshow about ' Percent Composition' - kaden-bradshaw

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### Percent Composition

### Empirical Formulas

Example: MgO

Find molar mass of whole compound:

MgO = 24.3 + 16.00 = 40.3 grams

% Mg (by mass) = mass of Mg = 24.3 g x 100 = 60.3%

molar mass of MgO 40.3 g

% O (by mass) = mass of O = 16.0 g x 100 = 39.7%

molar mass of MgO 40.3 g

Percent = part / whole

- 4Steps:
- Change the percent to grams
- Convert grams to moles
- Divide each of the moles by the smallest number to find the ratio
- Round ratio to a whole number. If the ratio is not a whole number (ex. 1.5) multiply each element by 2 to get a whole number

Gives the lowest whole-number ratio of elements and compounds in a formula

Examples

A compound contains 94.1% Oxygen and 5.9% Hydrogen. What is its empirical formula?

- 94.1% = 94.1g O
- 5.9% = 5.9g H

5.9g H

1 mol H

1 mol O

- 94.1g O

= 5.9 mol H

= 5.88 mol O

16 g O

1 g H

5.9

5.88

- 5.88
- 5.88

= 1.003

(can round to 1.0)

= 1.0

4) Ratio = 1:1 Formula = OH

Examples

A compound contains 67.6% Mercury and 10.8% Sulfur and 21.6% Oxygen. What is its empirical formula?

- 67.6% = 67.6g Hg
- 10.8% = 10.8g S
- 21.6% = 21.6g O

67.6g Hg = 0.336 mol Hg

10.8g S = 0.338 mol S

21.6g O = 1.35 mol O

- 0.336
- 0.336

0.338

0.336

1.35

0.336

= 1.00 Hg

= 1.00 S

= 4.02 O

4)Ratio = 1:1:4 Formula = HgSO4

Examples

What is the empirical formula for a compound containing 70.0% Fe and 30.0% O?

- 70.0% = 70.0g Fe
- 30.0% = 30.0g O

70.0g Fe = 1.25 mol Fe

30.0g O = 1.875 mol O

1.875

1.25

- 1.25
- 1.25

= 1.5 O

= 1.00 Fe

4) Ratio = 1 : 1.5

5) Mult ratio by 2 = 2 : 3

Formula = Fe2O3

Molecular Formulas

- Same as empirical formula, or a simple whole-number multiple of it

- Steps:
- Calculate the mass in grams of the empirical formula provided
- Divide the molar mass by the mass of the empirical formula
- Multiply this whole number ratio by the empirical formula

Examples

Calculate the molecular formula of the compound whose molar mass is 60.0g and empirical formula is CH4N.

1) CH4N = 12 + 4(1) + 14 = 30.0 g

- 60.0g
- 30.0g

= 2.0

3) 2.0 (CH4N)

= C2H8N2

Examples

What is the molecular formula of ethylene glycol (CH3O), used in antifreeze. It has a molar mass of 62 g/mol.

1) CH3O = 31.0 g

3) 2.0 (CH3O)

= C2H6O2

- 62.0g
- 31.0g

= 2.0

Find the molecular formula of C3H2Cl, which is mothballs. Its molar mass is 147 g/mol.

1) C3H2Cl = 73.0 g

3) 2.0 (C3H2Cl)

= C6H4Cl2

- 147.0g
- 73.0g

= 2.0

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