The order of a reaction with rate equals $k[C_A]^{3/2} [C_B]^{-1/2}$ is

$A$ substance undergoes first-order decomposition. The decomposition follows two parallel first-order reactions as:
$A \xrightarrow{k_1} B$ $k_1 = 1.26 \times 10^{-4} \ s^{-1}$
$A \xrightarrow{k_2} C$ $k_2 = 3.8 \times 10^{-5} \ s^{-1}$
The percentage distribution of $B$ and $C$ are:

State whether the following statements are true $(T)$ or false $(F)$.
$(a)$ In a pseudo first order reaction,the rate and rate constant are determined with respect to the reactant present in lower concentration.
$(b)$ The hydrolysis of an ester is carried out in the presence of an excess of water in an acidic medium.
$(c)$ The hydrolysis of an ester is a second order reaction.

For the reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be:

If the surface area of the reactants increases,then the order of the reaction:

For the reaction ${H_{2(g)} + I_{2(g)} \to 2HI_{(g)}}$,the possible mechanism is given below:
$I_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2 I$ (fast step)
${2I + H_2 \xrightarrow{K_2} 2HI}$ (slow step)
Determine the rate law for the reaction.