Problem: The decomposition of azomethane (C2H6N2) follows first-order kinetics with a rate constant of 40 min−1. If you start with a concentration of 0.2 M C2H6N2, what is the rate of the decomposition after 0.1 min? A. 1.46 × 10−1 M min−1B. 4 M min−1C. 4.46 × 102 M min−1D. 0.4 M min−1E. 3.66 × 10−3 M min−1

FREE Expert Solution

We are asked to calculate the rate of the decomposition after 0.1 min


The rate law for a first-order reaction is: 

rate = k[C2H6N2]


The integrated rate law for a first-order reaction is as follows:


ln[A]t = -kt + ln[A]o


where [A]t = concentration at time t, k = rate constant, t = time, [A]0 = initial concentration


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Problem Details

The decomposition of azomethane (C2H6N2) follows first-order kinetics with a rate constant of 40 min−1If you start with a concentration of 0.2 M C2H6N2, what is the rate of the decomposition after 0.1 min?

A. 1.46 × 10−1 M min−1

B. 4 M min−1

C. 4.46 × 102 M min−1

D. 0.4 M min−1

E. 3.66 × 10−3 M min−1

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