In a reaction with initially `0.12 M`, the concentration of reactant is reduced to `0.06 M` in `10` hour and to `0.03 M` in `20` hour. (i) What is order of reaction? (ii) What is rate constant? (b) The rate of a first order reaction is `0.04 mol litre^(-1) s^(-1)` at `10` minute and `0.30 mol litre^(-1)` at `20` minute after initiation. Find the half-life of the reaction.

In a reaction with initially `0.12 M`, the concentration of reactant i

1.	In a reaction with initially `0.12 M`, the concentration of reactant is reduced to `0.06 M` in `10` hour and to `0.03 M` in `20` hour. (i) What is order of reaction? (ii) What is rate constant? (b) The rate of a first order reaction is `0.04 mol litre^(-1) s^(-1)` at `10` minute and `0.30 mol litre^(-1)` at `20` minute after initiation. Find the half-life of the reaction.
Answer» Assuming I order, i.e., `K=2.303/t"log"_(10) a/((a-x))` For case `I: a=0.12 M, (a-x)=0.06 M, t=10 hr` `K=2.303/10"log"_(10)0.12/0.06=0.069 hr^(-1)` For Case `II: a=0.12 M, (a-x)=0.03 M, t=20 hr` `K=2.303/20"log"_(10)0.12/0.03=0.069 hr^(-1)` `:.` Reaction is of I order and rate constant `K=0.069 hr^(-1)` (b) Rate `=Kxx[A]` `0.04=K[A]_(10)` and `0.03=K[A]_(20)` `([A]_(10))/([A]_(20))=0.04/0.03=4/3` Also `t=2.303/K"log"([A]_(10))/([B]_(20))` when `t=10 min` `10=2.303/K"log" 4/3` `:. K=2.303/10"log"4/3=0.0288 min^(-1)` `t_(1//2)=0.693/K=0.693/0.0288=24.06 min`

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