- 115 Views
- Uploaded on
- Presentation posted in: General

The Mole & Formulas

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

The Mole & Formulas

Dr. Ron Rusay

Mole - Mass Relationships

Chemical Reactions

Stoichiometry

- The Mole
- % Composition: Determining the Formula of an Unknown Compound
- Writing and Balancing Chemical Equations
- Calculating the amounts of Reactant and Product
- Limiting Reactant

- The numberof carbon atoms in exactly 12 grams of pure 12C. The numberequals
6.02 10 23

- 1 mole of anything = 6.02 10 23 units
- 6.02 10 23“units” of anything: atoms, people, stars, $s, etc., etc. = 1 mole

Avogadro’s number equals 1 mole….which equals

6.022 1023 “units”

Counting by Weighing

12 red marbles @ 7g each = 84g

12 yellow marbles @4g each=48g

55.85g Fe = 6.022 x 1023 atoms Fe

32.07g S = 6.022 x 1023 atoms S

Relative Masses of 1 Mole

CaCO3

100.09 g

Oxygen

32.00 g

Copper

63.55 g

Water

18.02 g

- 1H weighs 1.6735 x 10-24 g and 16O 2.6560 x 10-23 g.
- DEFINITION: mass of 12C = exactly 12 amu.
- Using atomic mass units:

- 1 amu = 1.66054 x 10-24 g
- 1 g = 6.02214 x 1023 amu

E)

1.06

10

g

A mole of copper atoms has a mass of 63.55 g.

The mass of 1 copper atom is

63.55 g/(6.022

10

) = 1.06

10

g.

–

22

´

23

–

22

´

´

- Formula Weight a.k.a. Molecular Weight
- Formula weights (FW): sum of Atomic Weights (AW) for atoms in formula.
- FW (H2SO4) = 2AW(H) + AW(S) + 4AW(O)
- = 2(1.0 amu) + (32.0 amu) + 4(16.0)
- = 98.0 amu

- Molecular weight (MW) is the weight of the molecular formula in amu.
- MW of sugar (C6H12O6 ) = ?
- MW = 6(12.0 amu) + 12(1.0 amu) + 6(16.0 amu)
- = 180 amu

- A substance’s molar mass (equal to the formula weight: atomic or molecular weight in grams) is the mass in grams of one mole of the element or compound.
- C = 12.01 grams per mole (g/mol)
- CO2 = ??
- 44.01 grams per mole (g/mol)12.01 + 2(16.00) = 44.01

C)

46.07

The molar mass is the sum of masses of all the

atoms in the molecule.

2

12.01 + 6

1.008 + 1

16.00 = 46.07

´

´

´

C)

CH

Cl

The molar mass has units of g/mol.

(12.8 g/0.256 mol) = 50.0 g/mol. The molecule

with the closest molar mass is CH

3

Cl.

3

B)

278 g

The molar mass of sodium hydroxide, NaOH, is

22.99 g/mol + 16.00 g/mol + 1.008 g/mol = 40.00

g/mol. Convert to grams: 6.94 mol

(40.00 g/mol)

= 278 g.

´

- Mass percent of an element:
- For iron in (Fe2O3), iron (III) oxide = ?

E)

A

ll of these

The ratio of C to H in C

H

is 1:1. This is the

same ratio found for each of the compounds, so

all have the same percent composition by mass.

8

8

Morphine, derived from opium plants, has the potential for use and abuse. It’s formula is C17H19NO3. What percent, by mass, is the carbon in this compound?

42.5%

27.9%

71.6%

This cannot be solved until the mass of the sample is given.

Morphine, derived from opium plants, has the potential for use and abuse. It’s formula is C17H19NO3. What percent, by mass, is the carbon in this compound?

42.5%

27.9%

71.6%

This cannot be solved until the mass of the sample is given.

(17 12) / ((17 12) + (19 1) + (1 14) + 3 16)) = 0.716

0.716 100 = 71.6 %

C)

4.04 g

The molar mass of K

CrO

is 2

39.10 + 52.00 +

7

16.00 = 242.2. The mass fraction of potassium

is (2

39.10)/242.2 = 0.3229.

0.3229

12.5 g = 4.04 g.

´

2

7

´

´

´

- Dalton’s law of multiple proportions:
When two elements form different compounds, the mass ratio of the elements in one compound is related to the mass ratio in the other by a small whole number.

- Compound A contains:
1.000 g Sulfur & 1.500 g Oxygen

- Compound B contains:
1.000 g Sulfur & 1.000 g Oxygen

- Mass ratio A: 2 to 3; Mass ratio B: 1 to 1
- Adjusting for atomic mass differences: AW sulfur is 2x the AW oxygen; the atom ratios therefore are S1O3 and S1O2 respectively

- molecular formula = C6H6Benzene
- empirical formula = CH = C6/6H6/6
- molecular formula = (empirical formula)n
[n = integer] (CH)6

- Other representations: Lewis Dot formulas, structural formulas, 2-D, 3-D

Empirical Formulas from Analyses

- 1. Use percent analysis.
Let 100 % = 100 grams of compound.

- 2. Determine the moles of each element.
(Element % = grams of element.)

- 3. Divide each value of moles by the smallest of the mole values.
- 4.Multiply each number by an integer to obtain all whole numbers.

The dye indigo is a compound with tremendous economic importance (blue jeans wouldn’t be blue without it.) Indigo’s percent composition is: 73.27% C; 3.84% H; 10.68%N and 12.21% O. What is the empirical formula of indigo?

C6H4NO

C8H3NO

C8H5NO

I know this should be whole numbers for each atom, but I do not

know how to accomplish that.

The dye indigo is a compound with tremendous economic importance (blue jeans wouldn’t be blue without it.) Indigo’s percent composition is: 73.27% C; 3.84% H; 10.68%N and 12.21% O. What is the empirical formula of indigo?

C6H4NO

C8H3NO

C8H5NO

I know this should be whole numbers for each atom, but I do not

know how to accomplish that.

The Molecular Formula is the important objective.

The Molar Mass (molecular weight) must be determined in order to reach this objective since the Molar Mass may not be equal to the Empirical formula’s Mass.

The experimental process involves different processes as does the calculations.

Using mass percent data and molar mass is the most straightforward.

Combustion analysis is more involved.

COMPARISON of CALCULATIONS

Quinine:

C 74.05%, H 7.46%, N 8.63%, O 9.86%

- 74.05/12.01, 7.46/1.008, 8.63/14.01, 9.86/16.00
C6.166 H7.40 N0.616 O0.616

Empirical Formula Weight = ?

- Molecular Weight = 324.42
Molecular Formula = 2x empirical formula

A Mass Spectrometer

Records a mass spectrum

A mass spectrum records only positively charged

fragments

m/z = mass to charge ratio of the fragment

QUESTION

http://chemconnections.org/pdb/Quinine.html

From the structures, determine the

molecular formula of quinine.

A Carbon atom is at each angle.

Each C has 4 bonds (lines + Hs).

Hs are not always drawn in &

must be added.

A)C18H24NO2 B)C20H20NO3C)C20H24N2O2D)C20H26N2O2

ANSWER

http://chemconnections.org/pdb/Quinine.html

From the structures, determine the

molecular formula of quinine.

C = 20

H = 24

N = 2

O =2

A Carbon atom is at each angle.

Each C has 4 bonds (lines + Hs).

Hs are not always drawn in &

must be added.

C20H24N2O2

A)C18H24NO2 B)C20H20NO3C)C20H24N2O2D)C20H26N2O2

B)

C

H

8

8

The mass of CH is 13.018. 13.018 divides into

104.1 about 8 times. Therefore there are 8 CH

groups in this compound. C

H

is the molecular

8

8

formula.

Examine the condensed structural formulas shown below:

I) Acetic acid (main ingredient in vinegar), CH3COOH

II) Formaldehyde (used to preserve biological specimens), HCHO

III) Ethanol (alcohol in beer and wine), CH3CH2OH

For which molecule(s) are the empirical formula(s) and the molecular formula(s) the same?

A) II B) I and II C) II and III D) I, II, and III

Examine the condensed structural formulas shown below:

I) Acetic acid (main ingredient in vinegar), CH3COOH

II) Formaldehyde (used to preserve biological specimens), HCHO

III) Ethanol (alcohol in beer and wine), CH3CH2OH

For which molecule(s) are the empirical formula(s) and the molecular formula(s) the same?

A) II B) I and II C) II and III D) I, II, and III