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Unformatted text preview: Discussion 3 Chem002 Spring 2008 [1] At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen according to the reaction: 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) When the rate of formation of NO 2 is 5.5 104 M/s, (a) What is the rate of decomposition of N 2 O 5 in M/s? (b) What is the average rate of the reaction? [2] Explain how the rate will change when the concentration is doubled for exponents of x = 2, 1, 0, , 1, and 2 in the rate expression: rate = k[A] x [3] What is the rate law for aA + bB + cC D when the following data has been obtained. Rate [A] [B] [C] 0.0370 mol/Ls 0.0030 0.0030 0.0050 0.105 mol/Ls 0.0060 0.0060 0.010 0.210 mol/Ls 0.0060 0.012 0.020 0.210 mol/Ls 0.0060 0.12 0.020 What is the value of k, including units? What will the rate if [A] = [B] = [C] = 0.12 M Answers: [1] (a) rate of N 2 O 5 decomposition = rate of NO 2 formation, from the relation: 1/2( [N 2 O 5 ]/ t) = ( [NO 2 ]/ t). So, rate of N 2 O 5 decomposition = 2.8 10decomposition = 2....
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This note was uploaded on 04/17/2008 for the course CHEM 2 taught by Professor Ryan during the Spring '08 term at Marquette.
 Spring '08
 RYAN
 Reaction

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