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 ${\mathrm{O}}_2$?

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 $\mathrm{CO}$?