Lecture_Notes_082809b

# Lecture_Notes_082809b - Lecture Note 8/28/2009

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Method of Initial Rates y Initial rate data at 25 o C are listed in the table below for the reaction: { NH 4 + (aq) + NO 2 - (aq) Æ N 2(g) + 2 H 2 O (l) What is the rate law? Experiment [NH 4 + ][ N O 2 - ] Initial Rate (M/s) 1 0.24 M 0.10 M 7.2 x 10 -6 2 0.12 M 0.10 M 3.6 x 10 -6 3 0.12 M 0.15 M 5.4 x 10 -6

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Method of Initial Rates y What is the value of the rate constant? Experiment [NH 4 + ][ N O 2 - ] Initial Rate (M/s) 1 0.24 M 0.10 M 7.2 x 10 -6 2 0.12 M 0.10 M 3.6 x 10 -6 3 0.12 M 0.15 M 5.4 x 10 -6
Method of Initial Rates y What is the reaction rate when the concentrations are [NH 4 + ] = 0.39 M and [NO 2 - ] = 0.052 M?

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Method of Initial Rates y Using the information in the table below determine the rate law for the reaction: 2 NO (g) + 2 H 2 (g) N 2 (g) + 2 H 2 O (g) 0.0339 0.488 0.105 3 Experiment [NO] (M) [H 2 ] (M) Initial Rate (M/s) 1 0.420 0.122 0.136 2 0.210 0.122 0.0339
Method of Initial Rates y What is the rate constant for the reaction? 0.0339 0.488 0.105 3 Experiment [NO] (M) [H 2 ] (M) Initial Rate (M/s) 1 0.420 0.122 0.136 2 0.210 0.122 0.0339

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Method of Initial Rates y What is the initial rate of the reaction if [NO] = 0.350 M and [H 2 ] = 0.205 M?
Method of Initial Rates: Summary 1.

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## Lecture_Notes_082809b - Lecture Note 8/28/2009

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