Section 12.1. Stoichiometry. What is Stoichiometry?. Study of quantitative relationships between amounts of reactants used and products formed. Based on the Law of Conservation of Mass (Mass of the Reactants = Mass of the Products) Ex. 4 Fe (s) + 3 O 2 (g) 2 Fe 2 O 3 (s).
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Study of quantitative relationships between amounts of reactants used and products formed.
Based on the Law of Conservation of Mass (Mass of the Reactants = Mass of the Products)
Ex. 4 Fe (s) + 3 O 2 (g) 2 Fe2O3(s)
Coefficients in a balanced equation can be interpreted in
terms of representative particles and also by numbers of
moles of particles.
We can also use what we know about the conversion factor
that relates mass and number of moles to find the mass of
either the reactants or products.
Ex. 4 Fe (s) + 3 O2(g) 2 Fe2O3(s)
4 mol Fe x 55.85 g Fe = 223.4 g Fe
1 mol Fe
3 mol O2 x 32.00 g O2 = 96.0 g O2
1 mol O2
Mass of Reactants = 319.4 g
2 mol Fe2O3 x 158.7 g Fe203 = 319.4 g
1 mol Fe203
Mass of Products = 319.4 g
Ratio between the numbers of moles of any two substances in a balanced chemical equation.
Ex. 2 Al (s) + 3 Br2(l) 2 AlBr3(s)
2 mol Al and _2 mol Al_3 mol Br2 and _3 mol Br2_
3 mol Br2 2 mol AlBr3 2 mol Al 2 mol AlBr3
2 mol AlBr3 and 2 mol AlBr3
2 mol Al 3 mol Br2
What mole ratios can be written for the decomposition of potassium chlorate?
2 KClO3(s) 2 KCl (s) + 3 O2(g)
2 mol KClO3 and 2 mol KClO3
2 mol KCl 3 mol O2
_2 mol KCl_ and _2 mol KCl_
2 mol KClO3 3 mol O2
__3 mol O2_ and _3 mol O2
2 mol KClO3 2 mol KCl
2 H2 + O2 2 H2O
1. How many moles of water can be produced with 6 moles of hydrogen?
2. How many moles of oxygen would be required to fully react with 8 moles of hydrogen?
3. How many moles of water can be produced with 4 moles of oxygen?
4. How many moles of hydrogen would be required to produced 10 moles of water?
5. How many moles of oxygen would be needed to produce 20 moles of water?
(Example: Stoichiometry Practice II, # 4)
(Example: Stoichiometry Practice II, # 6)