For the reaction $2A + B \rightarrow \text{Product}$,the half-life period remains unchanged when the concentration of $B$ is doubled. However,when the concentration of $A$ is doubled,the rate of the reaction doubles. Determine the unit of the rate constant for this reaction.

For a reaction: $3X \to 4Y$,calculate the rate of reaction based on the following graph when the concentration of $X$ is $0.1 \ M$.

Reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$
Which is True $(T)$ and False $(F)$ in the following statement?
The order of this reaction is $10$.

$Zn + 2H^{+} \to Zn^{2+} + H_2$
The half-life period is independent of the concentration of zinc at constant $pH$. For the constant concentration of $Zn$,the rate becomes $100$ times when $pH$ is decreased from $3$ to $2$. Identify the correct statements $(pH = -\log [H^{+}])$:
$(A)$ $\frac{dx}{dt} = k[Zn]^0[H^{+}]^2$
$(B)$ $\frac{dx}{dt} = k[Zn][H^{+}]^2$
$(C)$ Rate is not affected if the concentration of zinc is made four times and that of $H^{+}$ ion is halved.
$(D)$ Rate becomes four times if the concentration of $H^{+}$ ion is doubled at constant $Zn$ concentration.

The value of $\frac{t_{0.875}}{t_{0.50}}$ for $n^{th}$ order reaction is

For the decomposition reaction $2NH_3(g) \rightarrow N_2(g) + 3H_2(g)$,if the rate constant $k = 2.6 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,calculate the rate of formation of $N_2$ and $H_2$.