Chapter 9. Section #3! Stoichiometry and Cars!
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1 Section #3! Stoichiometry and Cars!
2 CH 9 Section #3 An Air Bag Could Save Your Life q When inflated, air bags slow the motion of a person so that he or she does not strike the inside of a car with as much force during a high-speed collision. q You still need to wear your seat belt! F = ma KE = 1 2 mv2
3 CH 9 Section #3 An Air Bag Could Save Your Life q Stoichiometry is used by air-bag designers to ensure that air bags do not under inflate or over inflate. q The chemicals that inflate the air bag must be present in just the right proportions.
4 CH 9 Section #3 Stoichiometry and Safety Air Bags Some Facts: q q q q Airbag deployment takes between milliseconds. The blink of an eye is around 200 milliseconds The bag is traveling at around 200 mile per hour. The bag should not be used around children and short people The bag gets very hot.
5 CH 9 Section #3
6 CH 9 Section #3 Air Bag Chemical Reactions: 2NaN 3 (s) 2Na(s) + 3N 2 (g) + Energy Sodium Metal is dangerous! 6Na(s) + Fe 2 O 3 (s) 3Na 2 O(s) + 2Fe(s) + Energy Sodium Oxide is a Hazard! Na 2 O(s) + 2CO 2 (g) + H 2 O(g) 2NaHCO 3 (s) + Energy
7 CH 9 Practice Problem Set #3, #1 In an air bag deployment, grams of Sodium Azide (NaN 3 ) is completely decomposed.!! a. Write the balanced equation! b. Calculate the mass of Sodium metal produced! c. Calculate the mass of Nitrogen gas produced.!
8 CH 9 Practice Problem Set #3, #2 Using the mass of nitrogen gas from practice problem #1c, calculate the volume in liters of nitrogen gas produced in the reaction.! Density N2 = 0.92 g 1.00 L
9 CH 9 Practice Problem Set #3, #3 a. Write out the second airbag equation! b. Using the calculated mass of sodium metal found in practice problem #1b, calculate the amount of solid sodium oxide produced in the reaction.!
10 CH 9 Practice Problem Set #3, #4 Using the calculated mass of sodium metal found in practice problem #1b, calculate the amount of solid iron (III) oxide needed to react with all of the sodium metal.!
11 CH 9 Practice Problem Set #3, #5 a. Write out the third airbag equation. b. Using the calculated mass of solid sodium oxide found in practice problem #3, calculate the amount of solid sodium hydrogen carbonate produced in the reaction.
12 CH 9 Section #3 Octane: Formula C 8 H 18
13 Octane: C 8 H 18 CH 9 Section #3 q Relative Molar Mass: grams! q Percent Composition by Mass:! Carbon = 84.1% C! Hydrogen = 15.8% H! q Type of bonding: covalent (non-metal to non-metal)!
14 CH 9 Section #3 q Refined from crude oil q Octane is a hydrocarbon, meaning that its structure is entirely made up of carbon and hydrogen atoms. q Octane is a saturated hydrocarbon, or alkane. q An alkane is a hydrocarbon whose bonds are all single bonds to four other atoms. q Octane also is a normal alkane because it forms a straight chain of atoms in a zig-zag pattern.
15 Octane: C 8 H 18 CH 9 Section #3
16 CH 9 Practice Problem Set #3, # Kilograms of Octane C 8 H 18 reacts with Oxygen in a combustion reaction. Write and balance the chemical reaction.
17 CH 9 Section #3 Practice Problem # Kilograms of Octane C 8 H 18 reacts with Oxygen in a combustion reaction. Calculate the grams of Oxygen required for the complete reaction.
18 CH 9 Practice Problem Set #3, # Kilograms of Octane C 8 H 18 reacts with Oxygen in a combustion reaction. Calculate the grams of Carbon Dioxide produced in this reaction.
19 CH 9 Practice Problem Set #3, # Kilograms of Octane C 8 H 18 reacts with Oxygen in a combustion reaction. Calculate the grams of liquid Water produced in this reaction.
20 CH 9 Practice Problem Set #3, #10 Using the mass of oxygen you calculated in problem # 7, Calculate the Liters of Oxygen required for the complete reaction. Density O2 = 1.43 grams 1.00 liter
21 CH 9 Practice Problem Set #3, #11 Using the mass of water you calculated in problem # 9, calculate the milliliters of water produced in the reaction. (Density of water is 1.00 gram / 1.00 ml)
22 CH 9 Practice Problem Set #3, #12 Using the mass of oxygen you calculated in problem # 7, Calculate the liters of air (a mixture of many gases) required for the complete reaction. Air is 21 % oxygen by volume. 100 % air 21 % O 2
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