The variation of the rate of an enzyme catalyzed reaction with substrate concentration is correctly represented by graph

For the non - stoichimetre reaction $2A + B \rightarrow C + D,$ the following kinetic data were obtained in three separate experiments, all at $298\, K.$

The rate law for the formation of $C$ is :

The rate of reaction, $A + B + C \longrightarrow P$ is given by

$r = \frac{{ - d\left[ A \right]}}{{dt}} = K\,{\left[ A \right]^{\frac{1}{2}}}\,{\left[ B \right]^{\frac{1}{2}}}\,{\left[ C \right]^{\frac{1}{4}}}$

The order of reaction is

The reaction $2FeC{l_3} + SnC{l_2} \to 2FeC{l_2} + SnC{l_4}$ is an example of

The reaction $2NO + Br_2 \rightarrow  2NOBr,$ follows the mechanism given below

$(I)$  $NO + Br_2 \rightleftharpoons  NOBr_2 $    ........ Fast

$(II)$  $NOBr_2 + NO \rightarrow 2NOBr$     ......... Slow

The overall order of this reaction is

If a reaction has the experimental rate expression rate $= K [A]^2[B]$, if the concentration of $A$ is doubled and the concentration of $B$ is halved, the what happens to the reaction rate