Chemistry, 24.02.2020 18:41 kprincess16r
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 492 seconds, the concentration of CH3NC has decreased to 72% of its original value. Calculate the rate constant (k) of the reaction at 500. K.
Answers: 2
![\dfrac{d[CH_3NC]}{[CH_3NC]}=-kt](/tpl/images/0521/4081/74427.png)
![[CH_3NC]=[CH_3NC]_0e^{-kt}](/tpl/images/0521/4081/d933f.png)
![\dfrac{CH_3NC]}{[CH_3NC]_0}=0.72](/tpl/images/0521/4081/eda95.png)
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The isomerization reaction CH3NC → CH3CN obeys the first-order rate law, rate = k[CH3NC], in the pre...
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