For the following parallel chain reaction. What will be that value of overall half-life of $A$ in minutes ?

Given that  $\left[ {\frac{{{{\left[ B \right]}_t}}}{{{{[C]}_t}}} = \frac{{16}}{9}} \right]$

$A\,\xrightarrow{{{K_1}\, = \,2\, \times \,{{10}^{^{ - 3}\,}}{S^{ - 1}}}}4B$

$A\to C$

For the reaction $A + B \rightarrow$ products, it is observed that

$(i)\,\,$on doubling the initial concentration of $A$ only, the rate of reaction is also doubled and

$(ii)$  on doubling the initial concentration of both $A$ and $B,$ there is a change by a factor of $8$ in the rate of the reaction.

The rate of this reaction is given by

Rate of reaction is given by following rate law $ - \frac{{d\left[ c \right]}}{{dt}} = \frac{{{k_1}\,\left[ c \right]}}{{1 + {k_2}\,\left[ c \right]}}$ order of reaction when concentration is verh high

The rate of the reaction, $2NO + Cl_2 \rightarrow 2NOCl$ is given by the rate equation rate $= k[NO]^2[Cl_2].$ The value of the rate constant can be increased by

Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$

Which is True $(T)$ and False $(F)$ in the following sentence ?

The order of this reaction is $1$.

Consider following two reaction,

$A \to {\text{Product ;}}\,\, - \frac{{d[A]}}{{dt}} = {k_1}{[A]^o}$

$B \to {\text{Product ;}}\,\, - \frac{{d[B]}}{{dt}} = {k_2}{[B]}$

Units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as