A and B decompose via first order kinetics with half-lives 54.0 min and 18.0 min respectively. Starting from an equimolar non reactive mixture of A and B, the time taken for the concentration of A to become 16 times that of Bis______min. (Round off to the Nearest Integer).

A flask contains a mixture of compounds A and B . Both compounds decompose by first - order kinetics . The half - lives for A and B are 300 s and 180 s , respectively . If the concentration of A and B are equal initially , the time required for the concentration of A to be four times that of B (in s ) is : ( Use In 2 : 0.693)

There are two species A & B with half lives 54 & 18 minutes resp. The time after which concentration of A is 16 times that of B will be

A first order reaction is 20% complete in 10 min . Calculate (a) the specific rate constant of the reaction and (b) the time taken for the reaction to reach 75% completion.

A reaction has a half life of 1min. The time required for 99.9% completion of the reaction is .........min. (Round off to the Nearest Integer). [Use : ln =2 0.69, ln 10=2.3]

Half life of A is 54 min & half life of B is 18 min. Find the time when concentration of A = 16B

60% of a first order reaction was completed in 60 min . The time taken for reactants to decompose to half of their original amount will be

Two radioactive nuclides A and B have half-lives 50 min and 10 min respectively . A fresh sample contains the nuclides of B to be eight times that of A. How much time should elapse so that the mumber of nuclides of A becomes double of B ?

In a first order reaction, the concentration of the reactant decreases form 0.8 M to 0.4 M in 15 min . The time taken for the concentration to change form 0.1 M to 0.025 M is