For the reaction $X + Y \rightarrow Z$,the rate law is $r = K[X][Y]$. If the concentration of $Y$ is increased significantly,what will be the order of the reaction?

For the reaction $A + B \to C + D$,if the concentration of $A$ is doubled without affecting the concentration of $B$,the rate doubles. If the concentration of $B$ is increased $9$ times without affecting the concentration of $A$,the rate becomes $3$ times. Determine the order of the reaction.

The order of a reaction which has the rate expression $\frac{dc}{dt} = K[E]^{3/2}[D]^{3/2}$ is

$A$ 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 $1 \ hour$?

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 $K_3$?

If the concentration of the reactants is increased,the rate of reaction