For the reaction $2N_2O_{5(g)} \to 4NO_{2(g)} + O_{2(g)}$,what is the ratio of the rate of decomposition of $N_2O_5$ to the rate of formation of $NO_2$?

Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

For the elementary reaction $2 SO_{2(g)} + O_{2(g)} \rightarrow 2 SO_{3(g)}$,identify the correct relation among the following.

For the decomposition of $A$ as shown below,calculate the rate of appearance of $B$ if the initial concentration of $A$ is $2 \ M$.
$A_{(g)} \xrightarrow{K_1 = 2 \times 10^{-3} \ s^{-1}} 2B_{(g)}$
$A_{(g)} \xrightarrow{K_2 = 1 \times 10^{-3} \ s^{-1}} C_{(g)}$

Which are the units of rate of reaction?

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