Chemical Kinetics - Jensen Chemistry€¦ · The area of chemistry that concerns reaction rates...
Transcript of Chemical Kinetics - Jensen Chemistry€¦ · The area of chemistry that concerns reaction rates...
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The area of chemistry that concerns reaction rates (how fast a reaction occurs)
Unit 11.1
Chemical Kinetics
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Collision Model Key Idea: Molecules must collide to react.
However, only a small fraction of collisions produces a reaction. Why?
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Collision Model
Collisions must have sufficient energy to produce the reaction (must equal or exceed the activation energy).
Colliding particles must be correctly oriented to one another in order to produce a reaction.
1.
2.
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Endothermic Reactions
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Exothermic Reactions
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Factors Affecting Rate
Increasing temperature always increases the rate of a reaction.
Particles collide more frequently
Particles collide more energetically
Increasing surface area increases the rate of a reaction
Increasing Concentration (amount of reactants) USUALLY increases the rate of a reaction
Presence of Catalysts, which lower the activation energy by providing alternate pathways
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Catalysis •Catalyst: A substance that speeds up a reaction without being consumed
•Enzyme: A large molecule (usually a protein) that catalyzes biological reactions.
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Lowering of Activation Energy by a Catalyst
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Unit 11.2
Boiling points and phase diagrams
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Chemical Equilibrium
Reversible Reactions:
A chemical reaction in which the products can react to re-form the reactants
Chemical Equilibrium:
When the rate of the forward reaction equals the rate of the reverse reaction and the concentration of products and reactants remains unchanged
2HgO(s) 2Hg(l) + O2(g)
Arrows going both directions ( ) indicates equilibrium in a chemical equation
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Vapor pressure
• Vapor pressure of a liquid: pressure exerted by the liquid’s vapor at equilibrium
liquid + heat ↔ vapor
Higher temperatures = higher vapor pressures
Strong intermolecular forces = lower vapor pressures
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Vapor pressures of different compounds
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Boiling • Boiling occurs when a liquid’s vapor pressure = atmospheric
pressure.
• As the temp. of a liquid increases, its vapor pressure increases until it equals the outside pressure, this is when boiling starts
• In the mountains there is less atmospheric pressure so liquids will boil at a lower temp.
• Pressure cookers will increase the temp. at which liquids boil by increasing the outside pressure. Food can cook faster because the water is at a hotter temperature when boiling.
• Normal boiling point is the temp. liquids boil at sea level.
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Effect of Pressure on Boiling Point
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Phase Diagram Represents phases as a function of temperature and pressure.
Critical temperature: temperature above which the vapor can not be liquefied.
Critical point: critical temperature and pressure (for water, Tc = 374°C and 218 atm).
Triple point: where all three phases are in equilibrium
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Phase changes by Name
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Water
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Carbon dioxide Phase
Diagram for Carbon dioxide
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Carbon Phase
Diagram for Carbon
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Unit 11.3
Le Chatlier’s principle
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Chemical Equilibrium
Reversible Reactions:
A chemical reaction in which the products can react to re-form the reactants
Chemical Equilibrium:
When the rate of the forward reaction equals the rate of the reverse reaction and the concentration of products and reactants remains unchanged
2HgO(s) 2Hg(l) + O2(g)
Arrows going both directions ( ) indicates equilibrium in a chemical equation
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LeChatelier’s Principle
When a system at
equilibrium is placed under
stress, the system will
undergo a change in such
a way as to relieve that
stress.
Henry Le Chatelier
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When you take something away from a system at equilibrium, the system shifts in such a way as to replace what you’ve taken away.
Le Chatelier Translated:
When you add something to a system at equilibrium, the system shifts in such a way as to use up what you’ve added.
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LeChatelier Example #1
A closed container of ice and water at equilibrium. The temperature is raised.
Ice + Energy Water
The equilibrium of the system shifts to the _______ to use up the added energy.
right
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LeChatelier Example #2
A closed container of N2O4 and NO2 at equilibrium. NO2 is added to the container.
N2O4 (g) + Energy 2 NO2 (g)
The equilibrium of the system shifts to the _______ to use up the added NO2. left
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LeChatelier Example #3 A closed container of water and its vapor at equilibrium. Vapor is removed from the system.
water + Energy vapor
The equilibrium of the system shifts to the _______ to replace the vapor. right
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Lowering of Activation Energy by a Catalyst