iPad = 10:02 PM * 79% Chapter 14 Homework Set C: Attempt 2 * Question Completion

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iPad = 10:02 PM * 79% Chapter 14 Homework Set C: Attempt 2 * Question Completion Status: At a certain temperature, the decomposition of NO2 is second order with a rate constant of 2.85 M 'min''. If one starts with 1,23 M of NO2, how many minutes will it take for it to decompose to 0.577M? 5.00000 points Save Answer UESTION 2 Sucrose decomposes according to first order kinetics in an acidic solution with a rate constant of 0.216 h-1 at 25 °C. If one starts with 1.74 M of sucrose, how many hours will it take for 31.6% of it to decompose? (Be careful to recognize that the % is not what % remains!) 5.00000 points Save Answer UESTION 3 Sucrose decomposes according to first order kinetics in an acidic solution with a rate constant of 0.216 h-1 at 25 °C. If one starts with 2.29 M of sucrose, how many hours will it take for it to decompose to 29.4% of its initial value? Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save All Answers Close Window Save and Submit

Explanation / Answer

we have:
[NO2]o = 1.23 M
[NO2] = 0.577 M
k = 2.85 M-1.min-1

use integrated rate law for 2nd order reaction
1/[NO2] = 1/[NO2]o + k*t
1/(0.577) = 1/(1.23) + 2.85*t
1.7331 = 0.813 +2.85*t
2.85*t = 0.9201
t = 0.323 min
Answer: 0.323 min

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