Chapter 10: The Mole

Chapter 10: Chemical Quantities The Mole: A Measurement of Matter

3 Methods of Measuring Matter ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

What is the Mole? ,[object Object],[object Object],[object Object],A large amount!!!! VERY

HOLY “MOLE”LY ,[object Object],[object Object],[object Object],[object Object],[object Object]

[object Object],1 mole of hockey pucks would equal the mass of the moon! HOW LARGE IS IT??? 1 mole of basketballs would fill a bag the size of the earth!

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

Molar Mass Examples ,[object Object],[object Object],[object Object],12.01 g/mol 26.98 g/mol 65.39 g/mol

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

More Molar Mass Examples ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

D. Percentage Composition ,[object Object]

D. Percentage Composition ,[object Object], 100 = %Cu =  100 = %S = 79.852% Cu 20.15% S 127.10 g Cu 159.17 g Cu 2 S 32.07 g S 159.17 g Cu 2 S

[object Object],D. Percentage Composition %Fe =  100 = 78% Fe %O =  100 = 22% O 28 g 36 g 8.0 g 36 g

[object Object],D. Percentage Composition (38.0 g Cu 2 S)(0.79852) = 30.3 g Cu Cu 2 S is 79.852% Cu

[object Object],D. Percentage Composition  100 = %H 2 O = 24.51% H 2 O 36.04 g 147.02 g

Molar Conversions molar mass ( g/mol ) 6.02  10 23 ( particles/mol ) WHAT THE H*LL WAS THAT ALL ABOUT? MASS IN GRAMS MOLES NUMBER OF PARTICLES

Mr. Zehner, Can you show us some examples?

C. Molar Conversion Examples ,[object Object],26 g C 1 mol C 12.01 g C = 2.2 mol C

C. Molar Conversion Examples ,[object Object],2.50 mol 6.02  10 23 molecules 1 mol = 1.51  10 24 molecules C 12 H 22 O 11

C. Molar Conversion Examples ,[object Object],2.1  10 24 molecules 1 mol 6.02  10 23 molecules = 290 g NaHCO 3 84.01 g 1 mol

4 grams of He gas * 20 grams of Ne gas * 32 grams of O 2 gas * 46 grams of CO 2 gas * 1 mol of He gas * 1 mol of Ne gas * 1 mol of O 2 gas * 1mol of CO 2 gas *

What volume will 0.78 mol of H 2 occupy at STP? 0.78 mol H 2 x 1 1 mole 22.4 L = 17.47 L

A gaseous compound composed of oxygen has has a density of 2.14 g/L @ STP, what is the molar mass of the gas? 2.14 g L x 22.4 L mole = 47.9 g / mole

Emperical Formula ,[object Object],[object Object],[object Object]

Empirical Formula Example ,[object Object],25.9 g N x 1 mole N 14.01 g N 1 = 1.85 mol N 74.1 g O x 1 mole O 16.00 g O 1 = 4.63 mol O

Empirical Formula Example Cont. 1.85 mol N 4.63 mol O / 1.85 / 1.85 = = 1.00 2.50 x x 2 2 N 2 O 5 = = 2 5

Molecular Formula ,[object Object],[object Object],[object Object]

Chapter 10: The Mole

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Chapter 10: The Mole