# The Mole and Molar Mass

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2

2

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4

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## Mass of Ammonium Sulfate

The molar mass of ammonium sulfate is _______ g mol-1

The molar mass of acetic acid (CH3COOH) is ______ g mol-1

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We can use these equalities to construct conversion factors:

### Number of Atoms/Molecules

1 mol CH3COOH = 6.022 ×1023CH3COOH molecules ≡ 60.05 g CH3COOH

60.05 g mol CH3COOH 1 60.05 mol g CH3COOH 6.022 × 1023 molec. mol (CH3COOH) 6.022 × 1023 molec. mol (CH3COOH) 1

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×

### OR …

#grams of the element

per 100 grams of the compound.

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g/mol g/mol

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### oxygen).

– The organic compound is burned in oxygen.

– The products of combustion (usually CO2and H2O) are weighed.

– The amount of each element is determined from the mass of products.

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## Elemental Analysis Setup

The sample is burned in a stream of oxygen gas, producing … … H2O, which is absorbed by MgClO4, and … … CO2, which is absorbed by NaOH.

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## Elemental Analysis

(cont’d) If our sample were CH3OH, every two molecules of CH3OH …

… would give two molecules of CO2

… and four molecules of H2O.

12 Elemental analysis of butane (cooking gas) gave the following mass

composition:

C – 82.66%, H – 17.34%.

a) Determine the empirical formula of butane.

b) The molar mass of butane is 58.12 g/mol; what is the molecular formula?

Determine the empirical formula of phenol (a general disinfectant) from its elemental analysis:

C – 76.57% H – 6.43% H.

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• A chemical equation is a shorthand description of a chemical reaction, using symbols and formulas to represent the elements and compounds involved.

## Writing Chemical Equations

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### תואוושמ ןוזיא

• A balanced equation must conform to the law of conservation of mass! הסמ ה רומ יש קוח

• To balance an equation we need to adjust the

stoichiometric coefficients םיירטמ ויכיוטס ם י מדק מ

Balance the following equations:

H2+ O2→ H2O C2H6+ O2→ CO2+ H2O

Fe + O2→ Fe2O3

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• If an element is present in just one compound on each side of the equation, try balancing that element first.

• Balance any reactants or products that exist as the free element

last.

• In some reactions, certain groupings of atoms (such as

polyatomic ions) remain unchanged. In such cases, treat these groupings as a unit.

• At times, an equation can be balanced by first using a fractional coefficient(s). The fraction is then cleared by

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(g)

2(g)

3

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2

3

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### 1 mol CO

1 mol CO reacted per 2 mol H2 2 mol H2 reacted per 1 mol CO 1 mol CO was consumed per 1 mol CH3OH that evolved

1 mol CH3OH was formed for each 2 mol

of H2that reacted

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### Outline of Simple Reaction Stoichiometry

Stoichiometric factor (or: mole ratio)

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3

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2

2

2

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### Outline of Stoichiometry Involving Mass

To our simple stoichiometry scheme … … we’ve added a conversion from mass at the beginning … … and a conversion to mass at the end.

Substances A and B may be two reactants,

two products, or reactant and product.

Think: If we are given moles of substance A initially, do we need to convert

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dioxide with water; nitrogen monoxide is also produced.

How many grams of nitric acid are produced for every 5 kg of nitrogen dioxide that reacts?

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## Summary of Concepts

• Mass percent composition can be used to calculate the empirical formula.

– Additional information on the molecular weight of the material allows the calculation of the molecular formula

• A balanced equation must conform to the law of conservation of mass.

• Calculations involving reactions use stoichiometric factors based on stoichiometric coefficients in the balanced equation.

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## References

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