1. Chapter 12 Stoichiometry 12.1 The Arithmetic of Equations
12.2 Chemical Calculations
12.3 Limiting Reagent and
Percent Yield
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2. Take a worksheet and get started on it!
Chemical Equations
Do Now:
Take a worksheet and get started on it!
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3. Using Equations
Stoichiometry
Calculation of quantities of reactants and products in chemical reactions
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4. __N2(g) + __H2(g)  __NH3(g)
Using Equations
Balance the equation for producing ammonia.
__N2(g) + __H2(g)  __NH3(g)
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5. Writing and Using Mole Ratios
N2(g) + 3H2(g)  2NH3(g)
The three mole ratios derived from the balanced equation above are:
2 mol NH3
1 mol N2
3 mol H2
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6. Calculating Moles of a Product
Sample Problem 12.3
Calculating Moles of a Product
N2 + 3H2  2NH3
How many moles of NH3 are produced when 0.60 mol of nitrogen reacts with hydrogen?
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7. 2 mol NH3 0.60 mol N2  = 1.2 mol NH3 1 mol N2 Sample Problem 12.3
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8. Combustion of Gasoline
Chemical Equations
Combustion of Gasoline
2C8H O2  16CO2 + 18H2O ∆H = -10,224 kJ
How many moles of CO2 will be produced from the combustion of 30 moles of C8H18?
(note: 30 moles C8H18 is ~ 1 gallon of gasoline)
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9. 2H2(g) + O2(g) ↔ 2H2O(l) ∆H = -482 kJ
Chemical Equations
Combustion of Hydrogen / Electrolysis
2H2(g) + O2(g) ↔ 2H2O(l) ∆H = -482 kJ
How many moles of O2 are required to react with 10 moles of H2?
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10. END OF 12.1
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