For the reaction $A + B \rightarrow$ products, it is observed that

$(i)\,\,$on doubling the initial concentration of $A$ only, the rate of reaction is also doubled and

$(ii)$  on doubling the initial concentration of both $A$ and $B,$ there is a change by a factor of $8$ in the rate of the reaction.

The rate of this reaction is given by

Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$

Which is True $(T)$ and False $(F)$ in the following sentence ?

The order of this reaction is $1$.

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

For the first order decompsition reaction of $N_2O_5$, it is found that - 

$(a)$   $2N_2O_5\rightarrow\,\,4NO_2(g)+O_2(g)-\frac{d[N_2O_5]}{dt}=k[N_2O_5]$

$(a)$   $N_2O_5\rightarrow\,\,2NO_2(g)+1/2\,\,O_2(g)-\frac{d[N_2O_5]}{dt}=k'[N_2O_5]$

which of the following is true ?

In a reaction $2A + B \to {A_2}B$, the reactant $ A $ will disappear at

The mechanism for the reaction is given below $2P + Q \to S + T$ $P + Q \to R + S$(slow)$P + R \to T$ (fast)The rate law expression for the reaction is