In the phenomenon of autocatalysis,......

Match the column $I$ with column $II$ :

$a$. Rate constant for first order reaction	$i$. $mol \ lit^{-1} \sec^{-1}$
$b$. Molarity	$ii$. $\frac{k \times 1000}{M}$
$c$. Rate constant for zero order reaction	$iii$. $second^{-1}$
$d$. Limiting molar conductivity	$iv$. $\frac{\text{moles of solute}}{\text{Volume of solution (lit)}}$

Half-lives of a first order and a zero order reaction are same. Then the ratio of the initial rates of first order reaction to that of the zero order reaction is

The rate constant for the reaction $H_2 + I_2 \to 2HI$ is $k_1 = 49$. What is the rate constant for the reverse reaction $2HI \to H_2 + I_2$?

The decomposition of $N_2O_5$ follows first-order kinetics: $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$. Its half-life is $2.4 \ hours$. If $10.8 \ g$ of $N_2O_5$ is taken initially,how many liters of $O_2$ will be obtained at $STP$ after $9.6 \ hours$?

$A$ person's wound was exposed to some bacteria and then bacteria growth started to happen at the same place. The wound was later treated with some antibacterial medicine and the rate of bacterial decay $(r)$ was found to be proportional to the square of the existing number of bacteria at any instance. Which of the following set of graphs correctly represents the 'before' and 'after' situation of the application of the medicine?
[$Given: N = \text{No. of bacteria}, t = \text{time}$, bacterial growth follows $1^{st}$ order kinetics.]