For which type of reactions, order and molecularity have the same value ?

Write differential rate expression of following reaction and give its order of reaction :

$2 HI \rightarrow H _{2}+ I _{2}$

$2 NO _{( g )}+ O _{2( g )} \rightarrow 2 NO _{2( g )}$

The reaction $CH _{3} COF + H _{2} O \quad \rightleftharpoons CH _{3} COOH + HF$

Condition $I$ $:$ $\left[ H _{2} O \right]_{0}=1.00 \,M$

                           $\left[ CH _{3} COF \right]_{0}=0.01 \,M$

Condition $II$ $:$ $\left[ H _{2} O \right]_{0}=0.02 \,M$

                             $\left[ CH _{3} COF \right]_{0}=0.80 \,M$

Determine the order of reaction and calculate rate constant.

If $50\%$  of a reaction occurs in $100$ seconds and $75\%$ of the reaction occurs in $200$ seconds, the order of this reaction is

A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is 

$(i)$ doubled

$(ii)$ reduced to half $?$

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

  Which of the following are correct statements -

$(a)$  Rate constant of the reaction $10^{-4}$

$(b)$  Rate law of the reaction is $k[A][B]$

$(c)$  Rate of reaction increases four times on doubling the concentration of both the reactant