Chapter 12 blank - Zumdahl Chapter 12 CHEMICAL KINETICS What is a rate A change in something over time Definitions Chemical Kinetics Spontaneity

Chapter 12 blank - Zumdahl Chapter 12 CHEMICAL KINETICS...

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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 – y Spontaneity – y Reversibility –
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Definitions y Reaction Rate – y Average Rate – y Instantaneous Rate – y Half-life –
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y CLICKER QUESTION
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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 250 – 400 s
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Average Rate Δ [NO]/ Δ t (M/s) Time period (s) 0 – 50 s 50 – 100 s 100 – 150 s 150 – 200 s 200 – 250 s 250 – 400 s
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Average Rate Δ [O 2 ]/ Δ t (M/s) Time period (s) 0 – 50 s 50 – 100 s 100 – 150 s 150 – 200 s 200 – 250 s 250 – 400 s
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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)
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Using Rate Information y For the reaction 2 N 2 O 5 (g) Æ 4 NO 2 (g) + O 2 (g) , the following data were collected. Answer the following questions based on the experimental data. y a. The first half-life for this experiment is approximately ________________. y b. The second half-life for this experiment is approximately _____________. y c. The concentration of O 2 at 10 minutes is _________________________. y d. The concentration of NO 2 at 50 minutes is ________________________. y e. The rate of appearance of NO 2 is _______________ times the rate of appearance of O 2 . y f. The rate of appearance of NO 2 is __________ times the rate of disappearance of N 2 O 5 . 0.15 70 0.28 50 0.37 40 0.50 30 0.68 20 0.92 10 1.24 0 [N 2 O 5 ] (M) Time (min)
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Rate Law y Rate Law – y Order –
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Rate Law y Differential Rate Law – y Integrated Rate Law –
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Rate Law y The value of the rate constant depends on how the rate is defined.
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Rate Law
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Determining the Form of the Rate Law y Consider the reaction: { 2 N 2 O 5 (soln) Æ 4 NO 2 (soln) + O 2 (g) { We are given the following information: [N 2 O 5 ] (mol/L) Rate (mol/L*s) 0.90 5.4 x 10 -4 0.45 2.7 x 10 -4
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Method of Initial Rates y Initial Rate – y Method of Initial Rates –
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