For a certain reaction, the rate $$=\mathrm{k}[\mathrm{A}]^{2}[\mathrm{~B}]$$, when the initial concentration of A is tripled keeping concentration of $$\mathrm{B}$$ constant, the initial rate would

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R.

Assertion A : A reaction can have zero activation energy.

Reason R : The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy.

In the light of the above statements, choose the correct answer from the options given below:

For a chemical reaction

4A + 3B $$\to$$ 6C + 9D

Rate of formation of C is 6 $$\times$$ 10^$$-$$2 mol L^$$-$$1 s^$$-$$1 and rate of disappearance of A is 4 $$\times$$ 10^$$-$$2 mol L^$$-$$1 s^$$-$$1. The rate of reaction and amount of B consumed in interval of 10 seconds, respectively will be :

The given graph is a representation of kinetics of a reaction

The y and x axes for zero and first order reactions, respectively are