The gas-phase decomposition of CH3N2CH3, CH3N2CH3 C2H6(g) + N2(g), is studied at

Question

The gas-phase decomposition of CH3N2CH3, CH3N2CH3 C2H6(g) + N2(g), is studied at a certain temperature, giving the following data:
Time (s) [CH3N2CH3] (M)
0.0e+00 0.100
3.0e+03 0.0198
6.0e+03 0.00392
9.0e+03 0.000775
1.2e+04 0.000153


Figure out whether this reaction is first-order or second-order with respect to the concentration of CH3N2CH3. Calculate the value of the rate constant. Pick the choice from below which gives the correct reaction order and value of the rate constant for this reaction.

Please explain how you solved this! I really appreciate all help at this time!

Explanation / Answer

its a second order reaction 1/A=1/Ao +kt 1/0.0198=1/0.1+k 3*10^3 hence k=0.0135

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