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

For reaction :

$2NO_2(g) + O_3(g) \to N_2O_5(g) + O_2(g)$

rate law is $R = K\, [NO_2]' [O_3]'$.

Which of these possible reaction mechanisms is consistent with the rate law?

Mechanism $I :$

$NO_2(g) + O_3(g) \to NO_3(g) + O_2(g)$ (slow)

$NO_3(g) + NO_2(g) \to N_2O_5(g)$ (fast)

Mechanism $II :$

$O_3(g)  \rightleftharpoons  O_2(g) + [O]$ (fast)

$NO_2(g) + [O] \to NO_3$ (slow)

$NO_3(g) + NO_2(g) \to  N_2O_5$ (fast)

The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is

The data for the reaction $A + B \to C$ isThe rate law corresponds to the above data is

For a reaction, $A+B \rightarrow$ Product; the rate law is given by, $r=k[ A ]^{1 / 2}[ B ]^{2}$ What is the order of the reaction?

If doubling the concentration of a reactant $ 'A'$  increases the rate $4$ times and tripling the concentration of $'A' $ increases the rate $9$  times, the rate is proportional to