# Chapter 10: The Mole 1 mole = 6.02 x 10 23 particles A mole is also called Avogadros number.

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Chapter 10: The Mole 1 mole = 6.02 x 10 23 particles A mole is also called Avogadros number.

A paper clip is 3.2 cm in length. How many times can of mole of paper clips go around the Earth? (Circumference of the Earth is 25,000 miles, 1 in = 2.54 cm, 1 foot = 12 inches,1 mile = 5,280 feet)

6.02 x 10 23 particles – atoms, molecules, formula units P. 287-290

Conversions: Moles Particles, Particles Moles P.290-291 # of moles x 6.02 x 10 23 particles = particles mole # particles x mole = moles 6.02 x 10 23 particles

Freon - CCl 2 F 2 study sample problem 10.3 on p. 292 How many Fluorine atoms are in 5.5 moles of Freon? 5.5 mol of CCl 2 F 2 x 2 mol F Atoms = 11 mol of F atoms 1 mol of CCl 2 F 2

The Mass of a Mole of an Element P. 293-294 Conversions: moles mass, mass moles # of moles x # of grams = grams mole grams x mole = moles # of grams

The Mass of a Mole of a Compound P. 295-296 What is the molar mass of Potassium Chromate?

The Mole to Mass Relationship P.297-298 1.Find the molar mass of the compound. 2.Convert moles to grams by using molar mass as a conversion factor. Converting Moles to Mass - P. 298-299

Converting Mass to Moles of a Compound – P. 299

Particles Mass, Mass Particles Move through the mole tunnel.

Mole (tunnel) mass Units (atoms, molecules) 6.02 x 10 23 Molar Mass

Converting Mass to Particles

Calculating Percentage Composition P.305-307 % composition of an element = mass of element x 100% mass of compound 1.A compound is formed when 9.03 g of Mg combines with 3.48 g of N. What is the percent composition of the compound? 2.When a 14.2 g sample of mercury(II)oxide is decomposed into its elements by heating, 13.2 g of mercury is obtained. What is the percent composition of the compound? 3.Calculate the percentage composition of dicarbon hexahydride, sodium hydrogen sulfate and phosphoric acid.

Empirical Formula – The Simplest Formula P.309-310 Convert % grams (Assume 100 g) Convert grams moles Divide each mole quantity by the smallest mole quantity Cant have decimals

Convert grams moles Divide each mole quantity by the smallest mole quantity.

Determining Molecular Formula A True Formula P.311-312 1.Determine the empirical formula. 2.Divide the molar mass by the molar mass of the empirical formula.

Hydrates Opal – Silicon Dioxide an example of a hydrate Water is bonded to the atoms of the compound.

Desiccators Removes water from the surroundings. Circuitry. Electronics and optics. Calcium Sulfate Not soluble in alcohol Calcium Chloride

Naming Hydrates State the name of the substance and then add a prefix in front of the word hydrate Ex. Na 2 CO 3 * 10H 2 O – sodium carbonate decahydrate

Hydrated CoCl 2 11.75 g before heating Anhydrous CoCl 2 w/o water 9.25 g after heating Analyzing Hydrates

Find the mass of the water. Determine the moles of the compound and water. Divide by the smallest mole ratio.

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