Give one example of a fractional order reaction.

(b) $4 \mathrm{mol}$ of $\mathrm{A}$ and $3 \mathrm{mol}$ of $\mathrm{B}$ in $1500 \mathrm{mL}$ vessel.

(c) $0.4 \mathrm{mol}$ of $\mathrm{A}$ and $0.3 \mathrm{mol}$ of $\mathrm{B}$ in $100 \mathrm{mL}$ vessel.

For the reaction ${\mathrm{N}}_2+3{\mathrm{H}}_2⟶2{\mathrm{NH}}_3,$ the value of rate constant in the rate law for $-\frac{\mathrm{\Delta }\left[{\mathrm{H}}_2\right]}{\mathrm{\Delta t}}$ was found to be $0.48 \mathrm{L}{ \mathrm{mol}}^{-}{\mathrm{s}}^{-}$ What is the rate constant when the rate law is written as

(a) $-\frac{\mathrm{\Delta }\left[{\mathrm{N}}_2\right]}{\mathrm{\Delta t}}$

For the reaction, the value of the rate constant in the rate law for $-\frac{\mathrm{\Delta }\left[{\mathrm{H}}_2\right]}{\mathrm{\Delta t}}$was found to be $0.48 \mathrm{L}{ \mathrm{mol}}^{-}{\mathrm{s}}^{-}.$ What is the rate constant when the rate law is written as

(b) $\frac{\mathrm{\Delta }\left[{\mathrm{NH}}_3\right]}{\mathrm{\Delta t}}.$

Express the relationship between the rate of production of $\mathrm{NOCl}$ and the rate of disappearance of chlorine in the following reaction,

$2\mathrm{NO}+{\mathrm{Cl}}_2⟶2\mathrm{NOCl}$.

In a catalytic experiment involving the following reaction $2\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)⟶2{\mathrm{CO}}_2\left(\mathrm{g}\right),$ the average rate of reaction was measured as; rate $=\frac{\mathrm{d}\left[{\mathrm{CO}}_2\right]}{\mathrm{\Delta t}}=4\times {10}^{-3} \mathrm{mol}{ \mathrm{L}}^{-1}{\mathrm{s}}^{-1}$. What is the rate of reaction expressed in terms of ${\mathrm{O}}_2$?