Chapter 13 Lecture 2

# Chapter 13 Lecture 2 - 1 0.038 0.060 1.4 X 10 –5 2 0.076...

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Effects of Concentration on Reaction Rate (A funny thing happened on the way to equilibrium …) From Last time: For a general reaction: aA + bB + ••• cC + dD + ••• = + = + = = - = - = t D d t C c t B b t A a Rate ] [ 1 ] [ 1 ] [ 1 ] [ 1 Rates change over the course of the reaction Fast …. Slow

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Effects of Concentration on Rate given by: Rate Law: = n m B A k Rate ] [ ] [ k = rate constant m = 0,1,2,3,••• fractions n = 0,1,2,3,••• fractions [A], [B], Rate are “right now” Reaction order If n = 0 If n = 1 If n = 2
You get m and n by experiment. Initial Rate experiments Special time to look: [A] o , [B] o Early, near t = 0 n o m o B A k Rate ] [ ] [ = Why this time is so special S 2 O 8 2– + 3I 2SO 4 2– + I 3 Exper [S 2 O 8 2– ] [I ] Rate

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Unformatted text preview: 1 0.038 0.060 1.4 X 10 –5 2 0.076 0.060 2.8 X 10 –5 3 0.076 0.120 5.6 X 10 –5 Order of reaction with respect to each reagent and overall Find k Predict the rate of reaction if: [S 2 O 8 2– ] = 0.083; [I – ] =0.115 First Order Reactions: A → Products ] [ ] [ 1 1 ] [ 1 A k dt A d t A a Rate =-= ∆ ∆-= Do the math: Find t ½ when [A] = ½[A] o The idea of half life. Look at the piles First order Reaction: N 2 O 5 → 2NO 2 + ½O 2 Find rate constant, k If 2.50 g N 2 O 5 are initially present 1.50 g N 2 O 5 are present at t = 109s What is the half-life for the reaction? What mass of N 2 O 5 is present after 5 min?...
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Chapter 13 Lecture 2 - 1 0.038 0.060 1.4 X 10 –5 2 0.076...

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