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3. The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A]2. Assume k = 5.73 x 10-4 mol-1 L s-1. If the initial concentration of A is 0.19 mol L-1, what is the concentration of A (in mol L-1) after 5.41 minutes?

3. The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A]2. Assume k = 5.73 x 10-4 mol-1 L s-1. If the initial concentration of A is 0.19 mol L-1, what is the concentration of A (in mol L-1) after 5.41 minutes?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Tx 1. The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A]. Assume k = 14.08 x 10-5 s-1. If the concentration of A is 0.152 mol L-1 at 1.65 hours after the reaction starts, what was the concentration of A (in mol L-1) when the reaction started? 2. The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A] 2. If k= 9.6 x 10-4 mol-1 L s-1 and the initial concentration of A is 1.04 mol L-1, what is the half life of this reaction in minutes? 3. The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A]2. Assume k = 5.73 x 10-4 mol-1 L s-1. If the initial concentration of A is 0.19 mol L-1, what is the concentration of A (in mol L-1) after 5.41 minutes? 4. The rate constant of a chemical reaction is 6.56 s-1 at a temperature of 20.2 °C. If the activation energy is 45.8 kJ mol-1, what is the rate constant (in s- 1) at 50.6 °C?
Transcribed Image Text:Tx 1. The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A]. Assume k = 14.08 x 10-5 s-1. If the concentration of A is 0.152 mol L-1 at 1.65 hours after the reaction starts, what was the concentration of A (in mol L-1) when the reaction started? 2. The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A] 2. If k= 9.6 x 10-4 mol-1 L s-1 and the initial concentration of A is 1.04 mol L-1, what is the half life of this reaction in minutes? 3. The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A]2. Assume k = 5.73 x 10-4 mol-1 L s-1. If the initial concentration of A is 0.19 mol L-1, what is the concentration of A (in mol L-1) after 5.41 minutes? 4. The rate constant of a chemical reaction is 6.56 s-1 at a temperature of 20.2 °C. If the activation energy is 45.8 kJ mol-1, what is the rate constant (in s- 1) at 50.6 °C?
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