For a reaction $A \to$ Products, a plot of $log\,t_{1/2}$ versus $log\,a_0$ is shown in the figure. If the initial concentration of $A$ is represented by $a_0,$ the order of the reaction is

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

In a reaction $2A + B \to {A_2}B$, the reactant $ A $ will disappear at

Assertion : The kinetics of the reaction -

$mA + nB + pC \to m' X + n 'Y + p 'Z$

obey the rate expression as $\frac{{dX}}{{dt}} = k{[A]^m}{[B]^n}$.

Reason : The rate of the reaction does not depend upon the concentration of $C$.

Which of the following is correct

The reaction, $X + 2Y + Z \to  N$ occurs by the following mechanism

$(i)$ $X + Y  \rightleftharpoons  M$             very rapid equilibrium

$(ii)$ $M + Z \to  P$                        slow

$(iii)$ $O + Y \to  N$                       very fast

What is the rate law for this reaction