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:

Question

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: (A) (0.693/k) (B) (0.693/1/k) (C) (0.693/√2k) (D) not defined

Tardigrade Admin · Accepted Answer

Correct answer is (c) (0.693/√2k)

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

$\frac{0.693}{k}$

$\frac{0.693}{1/ k}$

$\frac{0.693}{2 k}$

not defined

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

Q. For the reaction A+2B→ products (started with concentrations taken in stoichiometric proportion), the experimentally determined rate law is: −dtd[A]​=k[A]​[B]​ The half life time of the reaction would be:

k0.693​

1/k0.693​

2k​0.693​