Molar Mass, Moles, and Molecules 7.3 Using Chemical Formulas.

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Presentation transcript:

Molar Mass, Moles, and Molecules 7.3 Using Chemical Formulas

What is a Mole?  A mole is a number used to describe a quantity of something, usually referring to mass, volume, or the number of particles.  As a unit, it is shortened to mol

Molar Mass  The atomic mass of an element on the periodic table is the mass of 1 mole of that element (also called the molar mass, measured in g/mol).  In a chemical formula, the subscript represents how many moles of that element are present in that compound.  Multiply the number of moles by the atomic mass to find the mass of an element in a compound.  Add together the masses of all elements in the compound to find the formula mass.

Formula Mass Examples 1. NaCl = 2. H 2 O = 3. CaSO 4 = Complete the practice problem on page 238.

Converting with Molar Mass  It is possible to find the number of moles of a given formula mass by dividing by the molar mass of each element in a formula.  Ex: How many moles of CO 2 are in g?  C =, O 2 =  Complete practice problem #1 and 3 on page 240.

Molecules  The quantity of a mole can also be used to find the number of particles of a substance are present (usually measured in molecules or atoms)  1 mole = x particles  This constant is known as Avogadro’s number.

Converting with Molecules  To find the number of molecules, multiply the number of moles by Avogadro’s number.  Ex: 1 mole of O 2 = ? Molecules  To find the number of moles, divide by Avogadro’s number.  Ex x10 24 molecules of O 2 = ? Moles  Complete practice problem #2 on page 242.

Mass, Moles, and Molecules  To convert between all three quantities, you must go through moles. (1 st divide, then multiply)  Ex: 4.04 g of H 2 = ? Molecules of H 2  Complete practice problem #2 on page 242.

Exit Ticket  P Complete #1-4 on the section review