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Jan_30_09

# Jan_30_09 - Chemistry 108 Friday Jan 30 Making Rate...

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Friday, Jan 30 Chemistry 108

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Making Rate Equations k 1 A B k -1 A: d[A]/dt = -k 1 [A] + k -1 [B] B d[B]/dt = + k 1 [A] – k -1 [B] Which one? Degree of Advancement (DOA) Rules: If rate involves product (right side), divide by stoichiometric coefficient and multiply by +1 If rate involves reactant (left side) divide by stoichiometric coeff and multiply by -1
2 DOA = +1/1 d[B]/dt = -1/1 d[A]/dt = + k 1 [A] – k -1 [B] For A ===== 2B DOA = -1/1 d[A]/dt = +1/2 d[B]/dt Problem: Given 2A → 3B and DOA = 0.15M/s, find d[B]/dt DOA = 0.15 = +1/3 d[B]/dt; d[B]/dt = 3x0.15M/s = 0.45M/s

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Other Rate Equations A → B → C k 1 k 2 d[A]/dt = -k 1 [A] d[B]/dt = +k 1 [A] – k 2 [B] d[C]/dt = k 2 [B]
Second Order/Bimolecular A + B → Product d[A]/dt = d[B]/dt = -k 1 [A][B] 1 st order in A, B second order overall Bimolecular DOA = +k 1 [A][B] Messy if A o ≠ B o , also if reversible

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. 2NO 2 ===== N 2 O 4 A = B DOA = k 1 [NO 2 ] 2 (soluble) H 2 + I 2 ===== 2HI Soluble if [H 2 ] o = [I 2 ] o DOA = k 1 [H 2 ] o 2
. 1/[A(t)] = 1/A o - k 1 t Y = b + mx Y = 1/[A(t)] b = 1/A o x =t m = -k

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Second Order Plot
Half Life 2 nd order • 1 st order same t 1/2 for each A

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Jan_30_09 - Chemistry 108 Friday Jan 30 Making Rate...

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