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Chapter 19 Reaction Rates And Equilibrium
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Rates Measures the speed of change over an interval of time
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Collision Theory Atoms, ions, and molecules can react to form products when they collide with enough kinetic energy.
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Activation Energy The minimum amount of energy that particles must have to react.
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Transition State The point at the peak of the activation energy where compounds change back to reactants or form new products.
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4 Factors affecting Reaction Rates 1.Temperature: Increase in temperature = increase in KE, w/more KE one has more and harder collisions causing more product to form
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2. Concentration More molecules means greater chance of collision resulting in the formation of new products.
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3. Particle Size (increased surface area) The more surface area you have the greater the chance of collision.
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4. Catalyst A substance that speeds up a reaction without being used up in that reaction. Usually written above the yields sign in an equation.
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Inhibitors Works against the catalyst.
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Reversible Reactions The reaction occurs in both directions at the same time.
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2 SO 2 + O 2 2 SO 3
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Chemical Equilibrium A state at which the forward and reverse reaction occur at the same rate.
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**DOES NOT MEAN** Same amount of product and reactant formed.
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LeChatlier’s Principle If stress is applied to a system in dynamic equilibrium, the system changes to relieve the stress.
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Concentration Increasing the concentration will always change the equilibrium away from the increased concentration.
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H 2 CO 3 CO 2 + H 2 O
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Temperature Equilibrium shifts in the direction that absorbs the heat
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2 SO 2 + O 2 2 SO 3 + Heat
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Pressure (in gasses) Only affects equilibrium if there is an unequal # of moles. Equilibrium moves to the side w/less moles.
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K (eq) Equilibrium Constant The lower case letters = # of moles of that compound aA + bB cC + dD
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K (eq) = [C] c x [D] d [A] a x [B] b
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K (eq) Equilibrium Constant It shows whether products or reactants are favored in the reaction. K (eq) > 1 Products are favored K (eq) < 1 Reactants are favored
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