The reaction $A \xrightarrow{K} \text{Product}$ is zero order while the reaction $B \xrightarrow{K} \text{Product}$ is first order. For what initial concentration of $A$,the half-lives of the two reactions will be equal?

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 $9.6 \ hours$?

An endothermic reaction with a high activation energy for the forward reaction is represented by the diagram:

The rate constant for the first order decomposition of $H_{2}O_{2}$ is given by the following equation:
$\log k = 14.34 - 1.25 \times 10^{4} \, K / T$
Calculate $E_{a}$ for this reaction and at what temperature will its half-period be $256 \, min$?

$t_{100\%}$ is the time required for the $100\%$ completion of the reaction, while $t_{1/2}$ is the time required for $50\%$ of the reaction to be completed. Which of the following options correctly represents the relation between $t_{100\%}$ and $t_{1/2}$ for zero and first-order reactions, respectively?

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	$iv$. $\frac{\text{moles of solute}}{\text{Volume of solution (lit)}}$