chapter_17-Lecture 2

chapter_17-Lecture 2 - Lecture 2 17-20 Chemical Equilibrium...

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Lecture 2 17-20
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hemical Equilibrium Chemical Equilibrium 17-21
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Reaching equilibrium on the macroscopic and molecular levels of the reaction: NO N 2 O 4 ( g ) 2NO 2 ( g ). 17-22
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Equilibrium of the N 2 O 4 -NO 2 system N 2 O 4 ( g )2 N O 2 ( g ) Ratio of the rate At equilibrium: rate fwd = rate rev constants is equal to the ratio of the concentration terms k fwd [N 2 O 4 ] eq = k rev [NO 2 ] eq Rearranging: 2 = k fwd k v [NO 2 ] eq q = K 2 Equilibrium Constant K fwd: the forward rate constant e reverse te constant rev [N 2 O 4 ] eq •[ N 2 O 4 ]: the concentration of N 2 O 4 O the concentration of NO 17-23 K rev: the reverse rate constant [NO 2 ]: the concentration of NO 2
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For a general reaction: ] o a ge e a eact o aA cC K = [C] c [A] a eq eq For an even more general reaction: A B C D [C] c [D] d eq eq aA + bB cC + dD K = [A] a [B] b eq eq This is also known as the LAW OF MASS ACTION . The values of a, b, c, d are those of the coefficients in the balanced chemical equation. hy subscript “ q”? 17-24 Why subscript eq ?
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For reaction at any arbitrary time ot necessary at equilibrium) (not necessary at equilibrium) For a general reaction a A+ b B c C+ d D d th i l ffi i t i th b l d ti ) ( a , b , c , and d are the numerical coefficients in the balanced equation) = [C] c [D] d
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This note was uploaded on 07/31/2010 for the course CHEM CHEM 01C taught by Professor Unknown during the Spring '10 term at UC Riverside.

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chapter_17-Lecture 2 - Lecture 2 17-20 Chemical Equilibrium...

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