The Mole Calculating Formula/Molar Mass Calculate the molar mass of carbon dioxide, CO 2. 12.01 g +...

The The MoleMole

Calculating Formula/Molar MassCalculating Formula/Molar MassCalculate the molar mass of carbon Calculate the molar mass of carbon dioxide, COdioxide, CO22..

12.01 g + 2(16.00 g) =12.01 g + 2(16.00 g) =44.01 44.01 gg

One mole of CO2 (6.02 x 1023 molecules) has a mass of 44.01 grams

Mole RelationshipsMole Relationships

Mole Mole

Atomsor

molecules

Atomsor

molecules

MassMass

6.02 X 1023 Atoms1 Mole

1 Mole

6.02 X 1023 Atoms

1 Mole

Molar Mass (g)

1 Mole

How would you convert,Atoms Moles Moles Atoms

Moles Mass (g) Mass (g) Moles

Mass (g) Atoms Atoms Mass (g)

6.02 x 1023

1 moles atoms

6.02 x 1023

1moles= = atoms

mole1moles=

1 mole

atoms6.02 x 1023

=atoms

atoms6.02 x 1023

1 mole

Calculations with Moles:Calculations with Moles:Converting moles to gramsConverting moles to grams

How many grams of lithium are in 3.50 moles of lithium?

3.50 mol Li= g Li

1 mol Li

7 g Li 24.524.5

Calculations with Moles:Calculations with Moles:Converting grams to molesConverting grams to moles

How many moles of lithium are in 18.2 grams of lithium?

18.2 g Li= mol Li

7 g Li

1 mol Li2.602.60

Calculations with Moles:Calculations with Moles:Using Avogadro’s NumberUsing Avogadro’s Number

How many atoms of lithium are in 3.50 moles of lithium?

3.50 mol

= atoms1 mol

6.02 x 1023 atoms 2.11 x 102.11 x 102424

Calculations with Moles:Calculations with Moles:Using Avogadro’s NumberUsing Avogadro’s Number

How many atoms of lithium are in 18.2 g of lithium?

18.2 g Li

= atoms Li

1 mol Li 6.02 x 1023 atoms Li

1.57 x 1024

7 g Li 1 mol Li

(18.2)(6.02 x 1023)/6.94

1 mol NaOH

40.00 g NaOH

• How many moles is 5.69 g of NaOH?

Na = 22.99 g/mol

O = 16.00 g/mol

H = 1.01 g/ mol 40.00 g/mol

5.69 g NaOH = 0.142 mol NaOH

• How many grams are in 9.45 mol of dinitrogen trioxide?

N2O3 = 2(14.01) + 3(16.00) = 76.02 g/mol

9.45 mol N2O3 76.02 g N2O3

1 mol N2O3

= 718.2 =718 g N2O3

Find the number of sodium ions, Na+, in 3.00 mol of Na2CO3

3.00 mol Na2CO3

2 mol Na+ 6.022 x 1023 ions

1mol Na2CO3 1 mol Na+

= 3.61 x 10 24 Na+ ions

Find the number of sodium ions, Na+, in 3.00 mol of Na4P2O7

3.00 mol Na4P2O7

4 mol Na+ 6.022 x 1023 ions

1mol Na4P2O7 1 mol Na+

= 7.23 x 1024 Na+ ions

Percent Composition, Empirical and Percent Composition, Empirical and Molecular FormulasMolecular Formulas

Courtesy www.lab-initio.com

7.3: Calculating Percent Composition of a Compound

• Like all percent problems: Part

• Find the mass of each component,

• then divide by the total mass (assume one mole).

100cmpd of mass

element of masselement of mass %

• What is the % composition of water.– Find MM: 2(1.01) + 16.00 = 18.02 g/mol

• Double check: %’s should add up to 100.

Percent Composition

%H =2.02 g H

18.02 g H2O 100 =

%O =16.00 g O

18.02 g H2O

11.2 % H

88.8 % O

What is the percent carbon in C5H8NO4

(MSG monosodium glutamate), a

compound used to flavor foods and

tenderize meats?

1. Find mass of C

1. 5 x 12.0 g = 60.0 g C

2. Find mass of MSG

1. 5(12.0) + 8(1.0) +14.0 +4(16.0)=146.0 g

3. Mass of element/ mass of cmpd x 100

1. 60.0 g C/146.0 g x100 = 41.1% C

Practice Problem

%Fe =28 g

36 g 100 =78% Fe

%O =8.0 g

36 g 100 =22% O

• Find the percentage composition of a sample that is 28 g Fe and 8.0 g O.– Determine total mass:

Percent Composition

28 g + 8.0 g = 36 g

Calculating Percentage CompositionCalculating Percentage CompositionCalculate the percentage Calculate the percentage composition of magnesium composition of magnesium carbonate, MgCOcarbonate, MgCO33..Formula mass of magnesium carbonate:Formula mass of magnesium carbonate:24.31 g + 12.01 g + 3(16.00 g) = 24.31 g + 12.01 g + 3(16.00 g) = 84.32 g84.32 g

100.00 100.00

%83.2810032.84

%24.1410032.84

%93.5610032.84

• How many grams of copper are in a 38.0-gram sample of Cu2S?

– Multiply mass of cmpd with % element

(38.0 g Cu2S)x(0.79852) = 30.3 g Cu

Using Percent as a Conversion Factor

Cu2S is 79.8% Cu (Sample 7-10 p 227)

B. Empirical Formula

reduce subscripts

• Smallest whole number ratio of atoms in a compound

EF vs MF

• Empirical Formula (EF)

• Def’n: lowest whole # ratio

• H2O

• HO• CH

• CH2O

• Molecular Formula (MF)

• Def’n: actual ratio

• H2O

• H2O2

• C6H6

• C6H12O6

Waterperoxid

ebenzenesugar

Calculating Empirical Formula

• It is not just the ratio of atoms, it is also the ratio of moles of atoms.

• In 1 mole of CO2 there is 1 mole of carbon and 2 moles of oxygen.

Steps for Calculating the Empirical Formula

We get a ratio from the percent composition.

Assume you have a 100 g sample.1. % = g

2. Convert grams to moles (÷ atomic mass)

3. Find lowest whole number ratio.

(÷ by smallest # of moles)

(if this step gives a decimal, multiply by 2, 3, or 4 to get whole #’s)

4. Use ratio to write the EF

• Calculate the empirical formula of a compound composed of 38.67 % C, 16.22 % H, and 45.11 %N.

Part 1 Calculate the number of moles

Assume 100 g• 38.67 g C x 1mol C = 3.220 mole C

12.01 g C • 16.22 g H x 1mol H = 16.09 mole H

1.01 g H• 45.11 g N x 1mol N = 3.219 mole N

14.01 g N

Part 2 calculate the formula!

3.220 mol C

16.09 mol H

3.219 mol N

1 mol C

5 mol H

1 mol N

Divide by the smallest number of moles

Empirical Formula• Find the empirical formula for a

sample of 25.9% N and 74.1% O.

25.9 g 1 mol

14.01 g = 1.85 mol N

74.1 g 1 mol

16.00 g = 4.63 mol O

1.85 mol

= 2.5 O

Empirical Formula

N1O2.5

Need to make the subscripts whole numbers multiply by 2

Try this!Try this!Adipic acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula of adipic acid?

carbonmolcarbong

carbonmolcarbong107.4

132.49

hydrogenmolhydrogeng

hydrogenmolhydrogeng78.6

oxygenmoloxygeng

oxygenmoloxygeng74.2

184.43

1. Convert to grams, calculate # of moles

2. Divide each value of moles by the 2. Divide each value of moles by the smallest of the values.smallest of the values.

Carbon:Carbon:

Hydrogen:Hydrogen:

Oxygen:Oxygen:

50.174.2

carbonmol

47.274.2

hydrogenmol

50.174.2

oxygenmol

3. Multiply each number by an 3. Multiply each number by an integer to obtain all whole numbers.integer to obtain all whole numbers.

Carbon: 1.50Carbon: 1.50 Hydrogen: 2.50Hydrogen: 2.50 Oxygen: 1.00Oxygen: 1.00x 2 x 2 x 2

33 55 22

Empirical formula:C3H5O2

Molecular Formula• “True Formula” - the actual number

of atoms in a compound

empiricalformula

molecularformula

Steps to calculating Molecular Formula1. Find the empirical formula.2. Find the empirical formula mass.3. Divide the molecular mass by the empirical mass.4. Multiply each subscript by the answer from step 3.

nmass EF

mass MF nEF

Molecular Formula• The empirical formula for ethylene is CH2. Find the

molecular formula if the molecular mass is 28.1 g/mol?

28.1 g/mol

14.03 g/mol = 2.00

empirical mass = 14.03 g/mol

(CH2)2 C2H4

1. Find the empirical formula and its mass

2. Divide the molecular mass by the empirical mass.

3. Multiply each subscript by the answer from step 3.

Finding the Molecular FormulaFinding the Molecular FormulaThe empirical formula for adipic The empirical formula for adipic acid is Cacid is C33HH55OO22. The molecular . The molecular mass of adipic acid is 146 g/mol. mass of adipic acid is 146 g/mol. What is the molecular formula of What is the molecular formula of adipic acid?adipic acid?

1. Find the formula mass of C1. Find the formula mass of C33HH55OO22

3(12.01 g) + 5(1.01) + 2(16.00) = 3(12.01 g) + 5(1.01) + 2(16.00) = 73.08 g73.08 g

Finding the Molecular FormulaFinding the Molecular Formula

3(12.01 g) + 5(1.01) + 2(16.00) = 3(12.01 g) + 5(1.01) + 2(16.00) = 73.08 g73.08 g

2. Divide the molecular mass by the empirical mass.

3. Multiply each subscript by the answer from step 3.

(C(C33HH55OO22) x ) x 22 = = CC66HH1010OO44

Example

• A compound is known to be composed of 71.65 % Cl, 24.27% C and 4.07% H. Its molar mass is known (from gas density) to be 98.96 g. What is its molecular formula?–EF: CClH2

–MF: C2Cl2H4

The Mole Calculating Formula/Molar Mass Calculate the molar mass of carbon dioxide, CO 2. 12.01 g +...

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