Which of the following statements is incorrect?

$A$ reaction between two different reactants cannot be a .....

Write the differential rate expression for the following reaction and determine its order of reaction:
$5 Br^{-} + BrO_3^{-} + 6 H^{+} \rightarrow 3 Br_2 + 3 H_2 O$

The following data is given for the reaction between $A$ and $B$:

$S.NO.$	$[A] \ mol \ L^{-1}$	$[B] \ mol \ L^{-1}$	$Rate \ mol \ L^{-1} \ sec^{-1}$
$I$	$1 \times 10^{-2}$	$2 \times 10^{-2}$	$2 \times 10^{-4}$
$II$	$2 \times 10^{-2}$	$2 \times 10^{-2}$	$4 \times 10^{-4}$
$III$	$2 \times 10^{-2}$	$4 \times 10^{-2}$	$8 \times 10^{-4}$

Which of the following are correct statements?
$(a)$ Rate constant of the reaction is $1 \ mol^{-1} \ L \ sec^{-1}$.
$(b)$ Rate law of the reaction is $k[A][B]$.
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactants.

The reaction $CH_{3}COF + H_{2}O \rightleftharpoons CH_{3}COOH + HF$ is studied under two conditions:
Condition $I$: $[H_{2}O]_{0} = 1.00 \ M$,$[CH_{3}COF]_{0} = 0.01 \ M$
Condition $II$: $[H_{2}O]_{0} = 0.02 \ M$,$[CH_{3}COF]_{0} = 0.80 \ M$

Time $(t)$ min (Condition $I$) / $[CH_{3}COF]$ $M$	Time $(t)$ min (Condition $II$) / $[H_{2}O]$ $M$
$0$ / $0.01000$	$0$ / $0.0200$
$10$ / $0.00867$	$10$ / $0.0176$
$20$ / $0.00735$	$20$ / $0.0156$
$40$ / $0.00540$	$40$ / $0.0122$

Determine the overall order of the reaction and calculate the rate constant.

The data for the reaction $A + B \to C$ is given below. The rate law corresponding to the above data is:

$Exp.$	$[A]_0$	$[B]_0$	Initial rate
$(1)$	$0.012$	$0.035$	$0.10$
$(2)$	$0.024$	$0.070$	$0.80$
$(3)$	$0.024$	$0.035$	$0.10$
$(4)$	$0.012$	$0.070$	$0.80$