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For a first order reaction, the rate con...

For a first order reaction, the rate constant is `6.909 "min"^(-1)`, the time taken for 75% conversion in minutes is

A

`((3)/(2))log2`

B

`((2)/(3))log2`

C

`((3)/(2))log((3)/(4))`

D

`((2)/(3))log((4)/(3))`

Text Solution

Verified by Experts

`k=((2.303)/(t))log(([A_(0)])/([A]))`
`[A_(0)]=100,[A]=25`
`6.909=((2.303)/(t))log((100)/(25))`
`t=((2.303)/(6.909))log(4)impliest=((1)/(3))log^(2)`
`t=((2)/(3))log^(2)`
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