For the reaction $2NO_2 + F_2 \to 2NO_2F$,the following mechanism has been provided:
$NO_2 + F_2 \xrightarrow{slow} NO_2F + F$
$NO_2 + F \xrightarrow{fast} NO_2F$
Thus,the rate expression of the above reaction can be written as:

For the first order decomposition reaction of $N_2O_5$,it is found that -
$(a)$ $2N_2O_5 \rightarrow 4NO_{2(g)} + O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$(b)$ $N_2O_5 \rightarrow 2NO_{2(g)} + 1/2 O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k'[N_2O_5]$
Which of the following is true?

Velocity constant $K$ of a reaction is affected by

Give two examples of zero-order reactions and two examples of first-order reactions.

$A$ bacterial infection in an internal wound grows as $N(t) = N_0 \exp(t)$,where the time $t$ is in hours. $A$ dose of antibiotic,taken orally,needs $1 \ hour$ to reach the wound. Once it reaches there,the bacterial population decreases as $\frac{dN}{dt} = -5N^2$. What will be the plot of $\frac{N_0}{N}$ vs. $t$ after $1 \ hour$?

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 $[B] = 0.2 \ M$.