Azomethane decomposes into nitrogen and ethane at elevated temperature:

H3C_N=N_CH3 _ N2 + C2H6

A chemist studying this reaction at 300ÁC begins an experiment with an azomethane concentration of 4.25 mM and obtains the following dаta:

Time (s) 100 150 200 250 300

[Azomethane] (mM) 3.29 2.90 2.55 2.25 1.98

Calculate the rate constant. Give an answer with concentration units of molarity and time units of seconds.

Question

Jay Marquez

Chemistry

7 November, 14:22

Azomethane decomposes into nitrogen and ethane at elevated temperature:

H3C_N=N_CH3 _ N2 + C2H6

A chemist studying this reaction at 300ÁC begins an experiment with an azomethane concentration of 4.25 mM and obtains the following dаta:

Time (s) 100 150 200 250 300

[Azomethane] (mM) 3.29 2.90 2.55 2.25 1.98

Calculate the rate constant. Give an answer with concentration units of molarity and time units of seconds.

+4

Answers (1)

Know the Answer?

Elliana · Answer 1

For a 1st order reaction:

In (n/n0) = - k * (time difference)

so k = - In (n/n0) / (t/t0)

n is concentration at time t and n0 is the concentration at an earlier time t0.

where k is constant.