$A_{(g)} + 2B_{(g)} \to$ product is an elementary reaction. Which of the following is incorrect?

For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?

The rate law for the reaction $A + B \rightarrow C$ at $25^{\circ} C$ is given by $\text{rate} = k[A][B]^2$. Calculate the rate of reaction if the rate constant at the same temperature is $6.25 \ mol^{-2} \ dm^6 \ s^{-1}$ where $[A] = 1 \ M$ and $[B] = 0.2 \ M$.

Consider the reaction between chlorine and nitric oxide:
$Cl_{2(g)} + 2NO_{(g)} \rightarrow 2NOCl_{(g)}$
On doubling the concentration of both reactants,the rate of the reaction increases by a factor of $8$. However,if only the concentration of $Cl_2$ is doubled,the rate increases by a factor of $2$. The order of this reaction with respect to $NO$ is :

$Zn + 2H^{+} \to Zn^{2+} + H_2$
The half-life period is independent of the concentration of zinc at constant $pH$. For the constant concentration of $Zn$,the rate becomes $100$ times when $pH$ is decreased from $3$ to $2$. Identify the correct statements $(pH = -\log [H^{+}])$:
$(A)$ $\frac{dx}{dt} = k[Zn]^0[H^{+}]^2$
$(B)$ $\frac{dx}{dt} = k[Zn][H^{+}]^2$
$(C)$ Rate is not affected if the concentration of zinc is made four times and that of $H^{+}$ ion is halved.
$(D)$ Rate becomes four times if the concentration of $H^{+}$ ion is doubled at constant $Zn$ concentration.

The rate law expression for the reaction $aA + bB \to P$ is $\text{rate} = K [A]^p [B]^q$. The order of the reaction is