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 $9.6 \ hours$?

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

Given below are two statements:
Statement $I$: The rate law for the reaction $A + B \rightarrow C$ is rate $(r) = k[A]^2[B]$. When the concentration of both $A$ and $B$ is doubled,the reaction rate is increased "$x$" times.
Statement $II$: The figure shows the variation in concentration against time plot for a "$y$" order reaction.
Concentration of $R$ vs Time plot: $A$ straight line with a negative slope equal to $-K$.
The value of $x + y$ is . . . . . .

Write the half-life $({t_{1/2}})$ equation and its unit for the following reactions:
$(i)$ Zero order reaction
$(ii)$ First order reaction

For a first order reaction,which of the following statements is correct?