question_answer

For the reaction \[A+2B\to \] products(started with concentrations taken in stoichiometric proportion), the experimentally determined rate law is \[-\frac{d[B]}{dt}=k\sqrt{[A]}\sqrt{[B]}\]

The half time of the reaction would be

A) \[\frac{\sqrt{2}\times 0.693}{k}\]            

B) \[\frac{0.693}{1/k}\]

C) \[\frac{0.693}{\sqrt{2}k}\]                     

D) not defined