For the reaction $A + 2B \rightleftharpoons 2C + D$,if the concentration of $A$ is increased four times and the concentration of $B$ is reduced to half,the rate of the reaction will be:

The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor of:

The following reactions occur for the reaction of $NO$ with $Br_2$ to form $NOBr$:
$NO_{(g)} + Br_{2_{(g)}} \rightleftharpoons NOBr_{2_{(g)}}$
$NOBr_{2_{(g)}} + NO_{(g)} \rightarrow 2 NOBr_{(g)}$
If the second reaction is the rate-determining step,the order of the reaction with respect to $NO_{(g)}$ will be:

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

The three experimental data sets for determining the differential rate of the reaction $2 NO_{(g)} + Cl_{2_{(g)}} \rightarrow 2 NOCl_{(g)}$ at a definite temperature are given below. (Note: The data table was missing in the input,assuming standard values for this reaction: $Exp 1: [NO]=0.1, [Cl_2]=0.1, Rate=0.18$; $Exp 2: [NO]=0.1, [Cl_2]=0.2, Rate=0.36$; $Exp 3: [NO]=0.2, [Cl_2]=0.1, Rate=0.72$).
$(a)$ Derive the differential rate law of the reaction.
$(b)$ Calculate the order of the reaction.
$(c)$ Calculate the value of the rate constant.

When the concentration of a reactant,$A$,in a reaction $A \to \text{Products}$ is doubled,the rate of reaction increases seven times. The order of the reaction is between: