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Unit 7: Stoichiometry Chapter 12.1 Pages

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**Stoichiometry Stoichiometry Greek for “measuring elements”**

Pronounced “stoy kee ahm uh tree” Definition: Calculations of the quantities in chemical reactions, based on a balanced equation.

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Stoichiometry There are 4 ways to interpret a balanced chemical equation Moles Coefficient ratios Particles 6.02 × 1023 particles/mole Mass Molar mass/mole Volume 22.4 L/mole

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Stoichiometry Mass and atoms are ALWAYS conserved, however, molecules, formula units, moles, and volumes will not necessarily be conserved

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**Stoichiometry Mole to Mole Conversions**

The coefficients tell us how many moles of each substance 2Al2O3 ® 4Al + 3O2 Molar Ratios Each time we use 2 moles of Al2O3 we also make 3 moles of O2. 2 moles Al2O3 3 mole O2 or

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**Stoichiometry 2Al2O3 ® 4Al + 3O2 Mole to Mole Conversions Practice**

How many moles of O2 are produced when 3.34 moles of Al2O3 decompose? 2Al2O3 ® 4Al + 3O2 3.34 mol Al2O3 2 mol Al2O3 3 mol O2 = 5.01 mol O2

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**Stoichiometry __Na + __H2O ® __NaOH + __H2 Mole to Mole Conversions**

Practice How many moles of H2 are produced when 2.05 moles of Na react with water? __Na + __H2O ® __NaOH + __H2 2.05 mol Na 2 mol Na 1 mol H2 = 1.03 mol H2

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Chapter 12 “Stoichiometry”

Chapter 12 “Stoichiometry”

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