If the rate constant $k = 4.5 \times 10^{-7} \text{ L}^2 \text{ mol}^{-2} \text{ s}^{-1}$, then what is the order of the reaction?

Give the relation between half-life $(t_{1/2})$ and initial concentration of reactant $([R]_0)$ for an $(n-1)^{th}$ order reaction.

The diazonium salt decomposes as $C_6H_5N_2^+Cl^- \to C_6H_5Cl + N_2$. At $0 \ ^\circ C$,the evolution of $N_2$ becomes two times faster when the initial concentration of the salt is doubled. Therefore,it is:

For the reaction $A + B \rightleftharpoons AB$,if the concentrations of both $A$ and $B$ are doubled,the rate of the reaction will become .......

The half-life periods of decomposition of $PH_3$ for different initial pressures are given below $:$

Initial Pressure $p$ (torr)	$707$	$79$	$37.5$
Half-life $t_{1/2}$ (min)	$84$	$84$	$84$

Determine the order of the reaction.

What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$