A first order reaction is 20% complete in the 10 minutes. Calculate the time period for 75% completion of the reaction.

Explanation

`K=(2.303)/(t) log""([A]_(0))/([A])" "`(First Order Reaction)
Let Initial Conc. `[A_(0)] = 100`
[A] = (100 - 20 = 80)
`k = (2.303)/(10) log"" (100)/(80)`
So,
`K = 0.0233 min^(-1)`
In second
Initial Conc. `[A_(0)] = 100`
[A] = 100 - 75 = 25
`t =(2.303)/(0.0233) log"" (100)/(25)`
t = 62.18 min.