The rate equation for the chemical reaction:
`aA+bB+cCrarreE+fF` is expressed as -
rate `=k[A]^(alpha)[B]^(beta)[C]^(0)`
Determine overall order and molecularity of the reaction.

Establish the rate equation for 1st order reaction.

For a reaction: H_(2)+Cl_(2)overset("hv")rarr2HCl, " rate"=K Write the order and molecularity of this reaction.

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 ?

Rate of the chemical reaction doubles for an increase of 10K from 298K . Calculate E_(a) .

The rate of the chemical reaction doubles for an increase of 10K in absolute temperature from 298K calculate E_a

Calculate the overall order of a reaction which has the rate expression : Rate =k[A]^(1//2)xx[B]^(3//2)

Calculate the overall order of a reaction which has the rate expression : Rate = k[A]^(3//2)xx[B]^(-1)

Write an account of the Arrhenius equation for rates of chemical reactions.

The rate constant for a zero order reaction aArarrbB is k. What is the rate of formation of B?

For a reaction : 2NH_(3)(g)overset("pt")rarrN_(2)(g)+3H_(2)(g),rate = K Write the order and molecularity of this reaction.