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General
Info
Chemical
Equation:
2CH3OH (l) + 3O2(g) à 2CO2(g) + 4H2O(g) + 736 kJ of heat energy
Liquid
methyl alcohol and gaseous oxygen react in a combustion reaction forming
gaseous carbon dioxide and gaseous water and 736 kilojoules of heat
energy.
Source
---- 1997 Zumdhal Chemistry, Boston, MA, Houghton Miffin Company pg.
120-121
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 1. What is this chemical reaction used for?
· Fuel for
powering cars
Source --- Source ---- 1997 Zumdhal
Chemistry, Boston, MA, Houghton Miffin Company pg. 120-121
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2.
How is the chemical reaction created?
·
The
reaction is created when a spark from the starter ignites the fuel
(methanol) in the presence of oxygen and creates a combustion reaction in
the engine
Source
---- 1997 Zumdhal Chemistry, Boston, MA, Houghton Miffin Company pg.
120-121, Self Interview
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3. How is
stoichiometry applied to this chemical reaction?
- Stoichiometry is applied when we
want to find out how much energy methanol is produced by a liter of
methanol in relation to a
liter of gasoline.
Source--- Personal Interview
4. Give a specific stoichiometric problem and
solve it for each reactant and product.
Ratio
of energy produced for gasoline and methanol.
Energy produced from the combustion of 1 liter
of methanol (CH3OH)
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1 liter CH3OH
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1000 mL CH3OH
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0.791 grams CH3OH
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1 mol CH3OH
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736 kJ
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= 20,000 kJ
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1 L CH3OH
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1 mL CH3OH
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32 grams CH3OH
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1 mol CH3OH
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Energy produced from the
combustion of 1 liter of gasoline[isooctane, (CH3)3CCH2CH(CH3)2].
2(CH3)3CCH2CH(CH3)2 + 25 O2 à 16 CO2
+ 18 H2O+10,900kJ
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1 liter (CH3)3CCH2CH(CH3)2
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1000 mL (CH3)3CCH2CH(CH3)2
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0.7 grams (CH3)3CCH2CH(CH3)2
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1 mol (CH3)3CCH2CH(CH3)2
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10,900 kJ
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10,900 kJ
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= 70,000 kJ
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1 liter (CH3)3CCH2CH(CH3)2
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1 mL (CH3)3CCH2CH(CH3)2
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114 grams (CH3)3CCH2CH(CH3)2
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1 mol
(CH3)3CCH2CH(CH3)2
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1 mol
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The ratio of energy for
gasoline to methanol is 70,000 to 20,000; therefore gasoline creates 350
percent more energy per liter.
Liters of oxygen required for
the combustion of 1 liter of methanol:
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1 liter CH3OH
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1000 mL CH3OH
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0.791grams CH3OH
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1 mols CH3OH
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3 mols O2
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32 grams O2
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1000mL O2
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1 liter CH3OH
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1 mL CH3OH
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32 grams CH3OH
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2 mols CH3OH
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1 mol O2
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1.429 grams O2
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1liter CH3OH
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= 800 liters O2
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1000 mL O2
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Therefore, the combustion of 1
liter of methanol requires 800 liters of oxygen.
Liters of C02
produced by the combustion of liter
of methanol:
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1 liter CH3OH
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1000 mL CH3OH
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0.791grams CH3OH
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1 mols CH3OH
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2 Mols C02
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44 Grams C02
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1 liter CH3OH
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1 mL CH3OH
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32 grams CH3OH
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2 Mols CH3OH
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1Mols C02
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1000 mL C02
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1 liter C02
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=500 liters C02
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2 grams C02
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1000 mL
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Therefore, 500 liters of CO2
are produced when methanol reacts with oxygen in a combustion
reaction.
Liters of H20
produced by the combustion of 1 liter of methanol:
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1 liter CH3OH
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1000 mL CH3OH
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0.791grams CH3OH
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1 mols
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1 liter CH3OH
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1 mL CH3OH
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32 grams CH3OH
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4 mols H20
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18 grams H20
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1mL H20
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1liter H20
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0.9 liters H20
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2 mols CH3OH
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1 mol H20
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1grams H20
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1000 mL H20
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Therefore, 0.9 liters of H20
are produced when methanol reacts with oxygen in a combustion reaction.
Source---2002 Chemistry in the Community, United States
of America, American Chemical Society pg 211, 2000 Holt Chemistry
Visualizing Matter Austin, Texas, Holt Rinehart and Winston pg. 370, 371,
1993 Modern Chemistry, Boca Raton, Florida, Dell Publishing Group page
290
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5.
Are any of your reactants normally the excess or limiting reactant?
Explain why.
- Methanol is the limiting reactant
and oxygen is the excess reactant because it is found all through
our atmosphere, while methanol is limited by the amount in the gas
tank.
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6. How much will the main chemical reaction
above cost to produce?
Cost for 1 liter of methanol (CH3OH):
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1 liter CH3OH
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5.25 dollars
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10.50 dollars
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.5 liter CH3OH
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Source---2002 Flinn Chemical &
Biological Catalog Reference Manual 2002 Batavia, IL, Flinn Science pg. 114
7. Are their any side reactions or dangers from
the original chemical reaction that must be compensated for? If yes, how is
it done?
- The reaction is a
combustion reaction so if the engine in the car were to malfunction,
there could be an explosion.
- This can be
prevented if the mechanic checks the engine to make sure it is safe to
run.
8. Bibliography
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- 1997 Zumdhal Chemistry, Boston,
MA, Houghton Miffin Company
pg. 120-121
- 2002 Chemistry
in the Community, United States of America, American Chemical
Society pg 211
- 2000 Holt
Chemistry Visualizing Matter Austin, Texas, Holt Rinehart and
Winston pg. 370,371
- 2002 Flinn
Chemical & Biological Catalog Reference Manual 2002 Batavia, IL,
Flinn Science pg. 114
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