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#39 A first-order reaction is 38. 5% complete in 480. s. a
#39 A first-order reaction is 38.5% complete in 480. s. a. Calculate the rate constant. b. What is the value of the half-life? c. How long will it take for the reaction to go to 25%, 75%, and 95% completion?
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a. Ln[A]= -Kt +Ln[A]o Ln[61. 5]= -K(480) + Ln[100] Ln[
a. Ln[A]= -Kt +Ln[A]o Ln[61.5]= -K(480) + Ln[100] Ln[.615]= -K(480) K=
![a. Ln[A]= -Kt +Ln[A]o Ln[61. 5]= -K(480) + Ln[100] Ln[](http://slideplayer.com./slide/13207775/79/images/2/a.+Ln%5BA%5D%3D+-Kt+%2BLn%5BA%5Do+Ln%5B61.+5%5D%3D+-K%28480%29+%2B+Ln%5B100%5D+Ln%5B.jpg "a. Ln[A]= -Kt +Ln[A]o Ln[61.5]= -K(480) + Ln[100] Ln[.615]= -K(480) K=")
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b. Ln[1/2]=-Kt +Ln[A]0 Ln[50]= (-0.00101)t + Ln[100] t=686 s
![b. Ln[1/2]=-Kt +Ln[A]0 Ln[50]= ( )t + Ln[100] t=686 s](http://slideplayer.com./slide/13207775/79/images/3/b.+Ln%5B1%2F2%5D%3D-Kt+%2BLn%5BA%5D0+Ln%5B50%5D%3D+%28+%29t+%2B+Ln%5B100%5D+t%3D686+s.jpg "b. Ln[1/2]=-Kt +Ln[A]0 Ln[50]= ( )t + Ln[100] t=686 s")
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c. Ln[A]= -Kt +Ln[A]o Ln[75]= (-0
c. Ln[A]= -Kt +Ln[A]o Ln[75]= ( )t + Ln[100] t= 280 s Ln[25]= ( )t + Ln[100] t= 1400 s Ln[5]= ( )t + Ln[100] t= 3000 s
![c. Ln[A]= -Kt +Ln[A]o Ln[75]= (-0](http://slideplayer.com./slide/13207775/79/images/4/c.+Ln%5BA%5D%3D+-Kt+%2BLn%5BA%5Do+Ln%5B75%5D%3D+%28-0.jpg "c. Ln[A]= -Kt +Ln[A]o Ln[75]= ( )t + Ln[100] t= 280 s Ln[25]= ( )t + Ln[100] t= 1400 s Ln[5]= ( )t + Ln[100] t= 3000 s.")
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