A follows first order reaction.
`(A) rarr Product`
The concentration of `A` changes form `0.1 M` to `0.025 M` in `40 min`. Find the rate of reaction of `A` when the concentration of `A` is `0.01 M`.

Options

A. (a) `3.47xx10^(-4) M//min`
B. (b) `3.47xx10^(-5) M//min`
C. (c ) `1.73xx10^(-4) M//min`
D. (d) `1.73xx10^(-5) M//min`

Answer

a

Explanation

For the first order reaction
`K=2.303/t"log"a/(a-x)`
`a=0.1 M, a-x=0.025 M, t=40 min`
`K=2.303/40"log"0.1/0.025`
`=2.303/40"log"4=0.0347 min^(-1)`
`[A] rarr` product
Thus, rate=`K[A]`
rate`=0.0347xx0.01 M min^(-1)`
`=3.47xx10^(-4) M min^(-1)`