# Lec 13 - 1 Problem from Last Time The reaction 2N 2 O 5 (g)...

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Unformatted text preview: 1 Problem from Last Time The reaction 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) The mechanism Step 1 fast: N 2 O 5 NO 2 + NO 3 Step 2 fast: N 2 O 5 NO 2 + NO 3 Step 3 slow:NO 2 + NO 3 NO 2 + O 2 + NO Step 4 fast: NO + NO 3 2NO 2 What is the rate law for this mechanism? A) Rate = k[NO 2 ][NO 3 ] B) Rate = k[N 2 O 5 ] C) Rate = k[NO][NO 3 ] D) Rate = k[N 2 O 5 ] 2 2 Mechanism Steps 1&2 fast: N 2 O 5 NO 2 + NO 3 Step 3 slow: NO 2 + NO 3 NO 2 + O 2 + NO Step 4 fast: NO + NO 3 2NO 2 Rate determined by the slow step Rate = k[NO 2 ][NO 3 ] Equilibrium is established in fast Steps 1&2 K eq = [NO 2 ][NO 3 ] / [N 2 O 5 ] Substitute [NO 2 ][NO 3 ] = K eq [N 2 O 5 ] So rate = k[N 2 O 5 ], which is (B) 3 Point of Confusion The rate of change of a reactant concentration is a negative number. [reactant]/ t = [final] – [initial] Reaction rates are always positive numbers. Rate = – [reactant]/ t A SmartWork question confused the two. 4 Catalysts A catalyst is a substance that increases the rate of a reaction but is not consumed in the reaction. It reacts and then is regenerated. Most catalysts used in the chemical industry are solid metal halide, metal oxides, or pure metals. 5 This graph contains the answers to all the questions about catalysts and how they work....
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## This note was uploaded on 06/20/2011 for the course CHEM 132 taught by Professor Laceyandhanson during the Spring '08 term at SUNY Stony Brook.

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Lec 13 - 1 Problem from Last Time The reaction 2N 2 O 5 (g)...

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