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11 Nov 2019


Can someone help me with part e? It’s throwing me off a bit

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Tod Thiel
Tod ThielLv2
30 Aug 2019

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1. A certain reaction has the following general form: aA → bB At a particular temperature and [A]0 = 4.00 × 10-3 M, concentration versus time data were collected for this reaction, and a plot of 1/[A] versus time result in a straight line with a slope value of +4.00 × 10-2 L/mol·s. a. Determine the differential rate law. b. Determine the integrated rate law. c. Determine the value of the reaction rate constant. d. Calculate the half-life, t½, for this reaction. e. How much time is required for the concentration of A to decrease to 1.00 × 10-3 M ?

2. One mechanism for the destruction of ozone in the upper atmosphere is: O3(g) + NO(g) → NO2(g) + O2(g) Slow NO2(g) + O(g) → NO(g) + O2(g) Fast Overall reaction: O3(g) + O(g) → 2O2(g) a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g) + O(g) → 2O2(g) is 14.0 kJ. Ea for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25 ºC? Assume that the frequency factor A is the same for each reaction.

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