011409 - 250 400 s Average Rate [NO]/ t (M/s) Time period...

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CHEMICAL KINETICS Zumdahl Chapter 12
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What is a rate? y A change in something over time.
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Definitions y Chemical Kinetics – the area of chemistry that concerns reaction rates and the steps through which a reaction occurs y Spontaneity – the inherent tendency for a process to occur, has nothing to do with the speed of the reaction y Reversibility – the ability of a reaction to go both forward and backward, it is often more favorable in one direction than in the other
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Definitions y Reaction Rate – change in concentration of a reactant or product per unit time y Average Rate – rate measured over a particular time period y Instantaneous Rate – rate measured at a specific time; determine instantaneous rate by taking the slope of the line tangent to the plot of [A] versus time
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Reaction Rate
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Reaction Rate
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Reaction Rate y What is happening when reaction is taking place?
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Average Rate - Δ [NO 2 ]/ Δ t (M/s) Time period (s) 0 – 50 s 50 – 100 s 100 – 150 s 150 – 200 s 200 – 250 s
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Unformatted text preview: 250 400 s Average Rate [NO]/ t (M/s) Time period (s) 0 50 s 50 100 s 100 150 s 150 200 s 200 250 s 250 400 s Average Rate [O 2 ]/ t (M/s) Time period (s) 0 50 s 50 100 s 100 150 s 150 200 s 200 250 s 250 400 s Average Rate 250 400 s 200 250 s 100 150 s 0 50 s [O 2 ]/ t (M/s) [NO]/ t (M/s) [NO 2 ]/ t (M/s) time period (s) Rate Law y Rate Law an expression that shows how the rate of a reaction depends on the concentration of the reactants y Order the exponent of the reactant concentrations, tells us how the rate depends on the concentrations of the reactants, has to be determined experimentally Rate Law y Differential Rate Law rate law that expresses how a rate depends on concentration, often just called the rate law y Integrated Rate Law rate law that expresses how concentration depends on time...
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011409 - 250 400 s Average Rate [NO]/ t (M/s) Time period...

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