1. Tardigrade
  2. Question
  3. Chemistry
  4. For the reaction A + 2B → products (started with concentrations taken in stoichiometric proportion), the experimentally determined rate law is: -(d[A]/dt)=k√[A]√[B] The half life time of the reaction would be:

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Q. For the reaction $A + 2B \to$ products (started with concentrations taken in stoichiometric proportion), the experimentally determined rate law is:
$-\frac{d\left[A\right]}{dt}=k\sqrt{\left[A\right]}\sqrt{\left[B\right]}$
The half life time of the reaction would be:

Chemical Kinetics

Solution:

Correct answer is (c) $\frac{0.693}{\sqrt{2k}}$

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