For the reaction,$N_2 + 3H_2 \rightarrow 2NH_3,$ if $\frac{d[NH_3]}{dt} = 2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1},$ the value of $-\frac{d[H_2]}{dt}$ would be .................. $mol \ L^{-1} \ s^{-1}$.

For the reaction $2 NH_{3(g)} \rightarrow N_{2(g)} + 3 H_{2(g)}$,the rate of disappearance of $NH_3$ is $1.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. What is the rate of formation of $N_2$ and $H_2$?

The reaction given below $2 NH_{3(g)} \xrightarrow{Pt} N_{2(g)} + 3 H_{2(g)}$ has a rate of reaction of $2.5 \times 10^{-6} \ mol \ dm^{-3} \ sec^{-1}$. What is the rate of formation of $H_{2(g)}$?

$KClO_3 + 6FeSO_4 + 3H_2SO_4 \rightarrow KCl + 3Fe_2(SO_4)_3 + 3H_2O$. The above reaction was studied at $300 \ K$ by monitoring the concentration of $FeSO_4$,where the initial concentration was $10 \ M$ and after half an hour it became $8.8 \ M$. The rate of production of $Fe_2(SO_4)_3$ is $........ \times 10^{-6} \ mol \ L^{-1} \ s^{-1}$.

Which of the following equations is correct regarding the rate of disappearance of reactant and appearance of product for the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$?

The velocity of disappearance for $HI$ is $2.4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. Calculate the rate of formation of $H_2$.