122ch14d_001

122ch14d_001 - 38 14.55) 39 14.57) 40 14.59) 41 14.60) 42...

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44 14.66) The decomposition of hydrogen peroxide is catalyzed by iodide ion and is thought to proceed by a two-step mechanism: H 2 O 2 (aq) + I & (aq) v H 2 O ( R ) + IO & (aq) (1) IO & (aq) + H 2 O 2 (aq) v H 2 O ( R ) + O 2 (g) + I & (aq) (2) -------------------------------------------------------------------- 2 H 2 O 2 (aq) + I & (aq) + IO & (aq) v 2 H 2 O ( R ) + IO & (aq) + O 2 (g) + I & (aq) Note : IO & and I & appear on both sides and will cancel (see b and c below). a) Write the rate law for each elementary step in the mechanism in terms of the reactants in that step. Step 1: r = k 1 [H 2 O 2 ] [I & ] Step 2: r = k 2 [H 2 O 2 ] [IO & ] b) Write the overall balanced equation for the reaction. Cancel things that appear on both sides of the equation above. 2 H 2 O 2 (aq) v 2 H 2 O ( R ) + O 2 (g) c) The intermediate is IO & (aq). Intermediates generally appear for the first time as a product in one step and used as a reactant in subsequent step. (It is produced and then consumed.) I & is a catalyst . Catalysts generally appear for the first time as a reactant and reproduced in a subsequent step as a product , so it can be used again and again. (It is consumed and reproduced.)
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This note was uploaded on 07/17/2008 for the course CHEM 122 taught by Professor Zellmer during the Summer '07 term at Ohio State.

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