Two substances A and B are present such that `[A_(0)]=4[B_(0]` and half-life of A is 5 minutes and that of B is 15 minutes. If they start decaying at the same time following first order kinetics after how much time the concentration of both of them would be same ?

Two reacants A and B are present such that [A_(0)] = 4[B_(0)] and t_(1//2) of A and B are 5 and 15 mintute respectively. If both decay folliwing I order, how much time later will concentrations of both of them would be equal?

In a 5 L container,3 moles of A are taken and it immediately starts decomposing with half-life of 10 minutes. After 10min, 3 moles of B are added which undergoes independent decomposition as A with half-life of 5 minutes. If both decompositions follow first order kinetics then how many minutes it will take for the concentration of A and B to become same from the time of start of decomposition of A ?

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

The half-life period of a first order reaction is 10 minutes. Starting with initial concentration 12 M, the rate after 20 minutes is

The half-life period of a first order reaction is 15 minutes. The amount of substance left after one hour will be: