Chemistry - Chp 10 - Chemical Quantities - PowerPoint

Chapter 10 “Chemical Quantities” Yes , you will need a calculator for this chapter!

Section 10.1 The Mole: A Measurement of Matter ,[object Object],[object Object]

How do we measure items? ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

What is the mole? We’re not talking about this kind of mole!

Moles (is abbreviated: mol) ,[object Object],[object Object],[object Object],[object Object]

Similar Words for an amount ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

What are Representative Particles? ,[object Object],[object Object],[object Object],[object Object],[object Object]

Types of questions ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],3 atoms of oxygen 12 (3 x 4) atoms of oxygen 3 total ions (1 Ca 2+ ion and 2 Cl 1- ions) 2 total ions (1 Na 1+ ion and 1 OH 1- ion) 5 total ions (2 Al 3+ + 3 SO 4 2- ions)

Practice problems ( round to 3 sig. figs .) ,[object Object],[object Object],[object Object],[object Object],2.75 x 10 24 molecules 0.0975 mol (or 9.75 x 10 -2 ) 4.44 x 10 24 atoms C 12.9 moles

Measuring Moles ,[object Object],[object Object],[object Object],[object Object]

Gram Atomic Mass (gam) ,[object Object],[object Object],[object Object],[object Object]

Examples ,[object Object],[object Object],[object Object],[object Object],28.1 grams C 1 mol Mg 8.72 x 10 22 atoms Li 13.6 grams U

What about compounds? ,[object Object],[object Object],[object Object],[object Object],[object Object]

Calculating Formula Mass Calculate the formula mass of magnesium carbonate, MgCO 3 . 24.3 g + 12 g + 3 x (16.00 g) = 84.3 g Thus, 84.3 grams is the formula mass for MgCO 3 .

Section 10.2 Mole-Mass and Mole-Volume Relationships ,[object Object],[object Object]

Molar Mass ,[object Object],[object Object],[object Object]

Examples ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],= 78 g/mol gram formula mass = 92 g/mol gram molecular mass = 12 g/mol gram atomic mass = 164 g/mol gram formula mass = 180 g/mol gram molecular mass = 149 g/mol gram formula mass

Since Molar Mass is… ,[object Object],[object Object],[object Object]

For example ,[object Object],[object Object]

For example ,[object Object],[object Object],[object Object]

For example ,[object Object],[object Object],[object Object],[object Object]

The Mole-Volume Relationship ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Standard Temperature and Pressure ,[object Object],[object Object],[object Object],[object Object],[object Object]

Practice Examples ,[object Object],[object Object],[object Object],= 103 L = 0.253 mol = 12.3 L

Density of a gas ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Practice Examples (D=m/V) ,[object Object],[object Object],[object Object],[object Object]

Another way: ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],= 44.0 g/mol = 64.0 g/mol m = D x V

Summary ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Section 10.3 Percent Composition and Chemical Formulas ,[object Object],[object Object]

Calculating Percent Composition of a Compound ,[object Object],[object Object],[object Object],[object Object],x 100 % = percent

Example ,[object Object],29.0 g Ag 33.3 g total X 100 = 87.1 % Ag 4.30 g S 33.3 g total X 100 = 12.9 % S Total = 100 %

Getting it from the formula ,[object Object],[object Object]

Examples ,[object Object],[object Object],[object Object],[object Object],[object Object],85.7% C, 14.3 % H 23.1% Al, 15.4% C, and 61.5 % O

Formulas ,[object Object],[object Object],Empirical formula : the lowest whole number ratio of atoms in a compound. Molecular formula : the true number of atoms of each element in the formula of a compound.

Formulas (continued) Formulas for ionic compounds are ALWAYS empirical (the lowest whole number ratio = cannot be reduced). Examples: NaCl MgCl 2 Al 2 (SO 4 ) 3 K 2 CO 3

Formulas (continued) Formulas for molecular compounds MIGHT be empirical (lowest whole number ratio). Molecular: H 2 O C 6 H 12 O 6 C 12 H 22 O 11 Empirical: H 2 O CH 2 O C 12 H 22 O 11 (Correct formula) (Lowest whole number ratio)

Calculating Empirical ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],= this is already the lowest ratio.

Calculating Empirical ,[object Object],[object Object],[object Object],[object Object],[object Object]

Example ,[object Object],[object Object],[object Object],[object Object],[object Object],Now divide each value by the smallest value

Example ,[object Object],[object Object],[object Object],[object Object],[object Object],= P 2 O 5 = C 4 H 5 N 2 O

Empirical to molecular ,[object Object],[object Object],[object Object],[object Object],= C 8 H 10 N 4 O 2

Note page 313 – Gas Chromatography used for chemical analysis

Chemistry - Chp 10 - Chemical Quantities - PowerPoint

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Chemistry - Chp 10 - Chemical Quantities - PowerPoint