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Molar Conversions in Chemistry: Understanding the Enormity of the Mole

Explore the concept of the mole in chemistry, its scale in terms of everyday objects, and how to convert between moles, grams, and representative particles using molar conversions. Examples included.

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Molar Conversions in Chemistry: Understanding the Enormity of the Mole

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  1. The Mole Molar Conversions

  2. A. What is the Mole? HOW LARGE IS IT??? • 1 mole of pennies would cover the Earth 1/4 mile deep! • 1 mole of hockey pucks would equal the mass of the moon! • 1 mole of basketballs would fill a bag the size of the earth!

  3. Molar Conversions Converting from moles to grams to representative particles and vice versa. Use the following conversion factor: 1 mole = 6.02 x 1023 representative units = molar mass (g) or formula weight Representative units - a. ionic compounds are called formula units b. molecular compounds are called molecules c. atoms are called atoms. Example of representative units - 6.02 x 1023 atoms Cu 6.02 x 1023 molecules O2 6.02 x 1023 units NaCl

  4. Molar Conversion Examples • How many moles of carbon are in 26.0 g of carbon? 26.0 g C 1 mol C 12.0 g C = 2.17 mol C

  5. Molar Conversion Examples • How many molecules are in 2.50 moles of C12H22O11? 6.02  1023 molecules 1 mol C12H22O11 2.50 mol C12H22O11 = 1.51  1024 molecules C12H22O11

  6. Molar Conversion Examples • Find the mass of 2.1  1024 formula units of NaHCO3. 2.1  1024 units NaHCO3 84.0 g NaHCO3 6.02  1023 units NaHCO3 = 290 g NaHCO3

  7. Molar Conversion Examples • Find the number of units of Iron (III) Chlorate in of 98.6 g of Iron (III) Chlorate. 6.02 x 1023 units Fe(ClO3)3 306.3 g Fe(ClO3)3 98.6 g Fe(ClO3)3 = 1.94 x 1023 units Fe(ClO3)3

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