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

 Which of the following statements is false ?

For the reaction, $2N_2O_5 \to 4NO_2 + O_2$ rate and rate constant are $1.02 \times 10^{-4}\, mol\,L^{-1}\,s^{-1}$ and $3.4 \times10^{-5}\,s^{-1}$ respectively. The concentration of $N_2O_5$ in $mol\,L^{-1}$ will be

For the reaction : $2A + B \to  A_2B$ ; the rate $= K[A]\, [B]^2$ with $K = 2.0\times10^{-6}\, lit^2\, mol^{-2}\, sec^{-1}$. Initial concentration of $A$ and $B$ are $0.2\, mol/lit$ and $0.4\, mol/lit$ respectively. Calculate the rate of reaction after $[A]$ is reduced to $0.12\, mol/litre$.

In a reaction involving hydrolysis of an organic chloride in presence of large excess of water$RCl + {H_2}O \to ROH + HCl$

In a reaction, the concentration of reactant is increased two times and three times then the increases in rate of reaction were four times and nine times respectively, order of reaction is