For the first order reaction `A to B`, deduce the integrated form of rate law.

In case of first order reaction -

For the first order reaction, rate constant depends upon

With the help of a graphical representation explain how the rate of a first order reaction varies with the initial concentration of reactant.

A first order reaction takes 10min to complete 40% of the reaction. Another first order reaction requires 15min to complete 60% of the reaction. Calculate the ratio of the rate constants of the two reactions.

The half life period of a first order reaction is 10 minutes. Then its rate constant is

Calculate the rate constant for a first order reaction if 90% of the reactant is converted to product in 100 minutes.

The rate constant of a first order reaction becomes 6 times when the temperature is raised from 350 K to 410K. Calculate the energy of activation for the reaction.

For the reaction : aA+bBrarrcC , the rate law is , r=k[A]^(m)[B]^(n) . If the initial concentration of A and B are doubled, then find the ratio of the new initial rate to the original initial rate.

The suggested mechanism of a reaction is : (a) A+BhArrD("fast) " (b)A+Drarr2C("slow") Write the balanced equation of the reaction if its experimentally deduced rate equation is , rate k=[A]^(2)[B] Find the intermediate formed during the course of the reaction . Does the predicted rate law from the mechanism match the experimental rate law ?