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For a first order reaction -(d[A])/(dt)=...

For a first order reaction `-(d[A])/(dt)=K[A]_(0)`. The reaction is carried out by taking `100 mol//litre` of A, then concentration of `A` decayed after time `1/K` is:

A

`36.79 mol litre^(-1)`

B

`61.21 mol litre^(-1)`

C

`26.79 mol litre^(-1)`

D

`53.21 mol litre^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
b
`[A]=[A]_(0)e^(-Kt)=[100]e^(-K//K)`
`=([100])/(e)=100/2.718=36.79 mol litre^(-1)`
`:. [A]_("decayed")=61.21`
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