For a reaction, $AB_5 \to AB + 4B$ The rate can be expressed in following ways

$\frac{{ - d[A{B_5}]}}{{dt}} = K[A{B_5}]$ ;    $\frac{{d[B]}}{{dt}} = {K_1}[A{B_5}]$

So the correct relation between $K$ and $K_1$ is

Which of the following rate laws has an overall order of $0.5$  for reaction involving substances $x$, $y$ and $z$

If initial concentration is reduced to its $1/4^{th}$  in a zero order reaction, the time taken for half of the reaction to complete

For a reaction $X + Y \to Z$, rate $ \propto \, [X]$. What is $(i)$ molecularity and $(ii)$ order of reaction ?

The order of the reaction occurring by following mechanism should be

$(i)$ ${A_2} \to A + A$ (fast)

$(ii)$ $A + {B_2} \to AB + B$ (slow)

$(iii)$ $A + B \to $ (fast)

In a chemical reaction $A$ is converted into $B$ . The rates of reaction, starting with initial concentrations of $A$ as $2 \times {10^{ - 3}}\,M$ and $1 \times {10^{ - 3}}\,M$ , are equal to $2.40 \times {10^{ - 4}}\,M{s^{ - 1}}$ and $0.60 \times {10^{ - 4}}\,M{s^{ - 1}}$ respectively. The order of reaction with respect to reactant $A$ will be