$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$

Initial $[A_2]$	Initial $[B_2]$	$R.O.R. (r) \ M s^{-1}$
$0.2$	$0.2$	$0.04$
$0.1$	$0.4$	$0.04$
$0.2$	$0.4$	$0.08$

Order of reaction with respect to $A_2$ and $B_2$ are respectively:

Consider the following gas-phase reaction.
$2HI_{(g)} \longrightarrow H_{2(g)} + I_{2(g)}$
and the following experimental data obtained at $555 \ K$. What is the order of the reaction with respect to $HI_{(g)}$?

$[HI] \ (M)$	Rate $(M \ s^{-1})$
$0.0500$	$8.80 \times 10^{-10}$
$0.1000$	$3.52 \times 10^{-9}$
$0.1500$	$7.92 \times 10^{-9}$

The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -
Step-$1$ : $A + E \rightleftharpoons AE$ (fast)
Step-$2$ : $AE + A \to A_2 + E$ (slow)
Step-$3$ : $A_2 + B \to C + D$ (fast)
What rate law best agrees with this mechanism?

The rate constant of a first order reaction at $27^{\circ} C$ is $10^{-3} \ min^{-1}$. The temperature coefficient of this reaction is $2$. What is the rate constant (in $min^{-1}$) at $17^{\circ} C$ for this reaction?

For the reaction,$2A + B \to \text{products}$,when the concentrations of $A$ and $B$ both were doubled,the rate of the reaction increased from $0.3 \ mol \ L^{-1} \ s^{-1}$ to $2.4 \ mol \ L^{-1} \ s^{-1}$. When the concentration of $A$ alone is doubled,the rate increased from $0.3 \ mol \ L^{-1} \ s^{-1}$ to $0.6 \ mol \ L^{-1} \ s^{-1}$. Which one of the following statements is correct?

State whether the following sentences are true $(T)$ or false $(F)$:
$(a)$ There is more than one reactant in a pseudo first order reaction.
$(b)$ In a pseudo first order reaction,the concentration of both reactants is the same.
$(c)$ In a pseudo first order reaction,the concentration of one reactant is very high.