The isomerization reaction CH3NC → CH3CN obeys the first-order rate law,  rate = k[CH3NC],  in the presence of an excess of argon. Measurement at 500. K reveals that in 485 seconds, the concentration of CH3NC has decreased to 73% of its original value. Calculate the rate constant (k) of the reaction at 500. K.   s−1

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The isomerization reaction CH3NC → CH3CN obeys the first-order rate law, 

rate = k[CH3NC],

 in the presence of an excess of argon. Measurement at 500. K reveals that in 485 seconds, the concentration of CH3NC has decreased to 73% of its original value. Calculate the rate constant (k) of the reaction at 500. K.

  s−1



(The integrated form for the first-order rate law can be written in the general terms 

ln[A]t − ln[A]0 = −kt,

 where 

[A]0

 is the initial concentration of reactant A, 

[A]t

 is the concentration of A at time t, and k is the rate constant.)

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