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 $NO_2$?

For the reaction,$NO_{2(g)} + CO_{(g)} \rightarrow NO_{(g)} + CO_{2(g)}$,the rate of formation of $NO_{(g)}$ is $Y$ (in $mol \ dm^{-3} \ s^{-1}$). Find the rate of disappearance of $CO_{(g)}$ (in $mol \ dm^{-3} \ s^{-1}$)?

Assertion : The rate of the reaction is the rate of change of concentration of a reactant or a product.
Reason : Rate of reaction remains constant during the course of reaction.

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the reaction occurs under specific temperature and partial pressure conditions. The rate of formation of $NH_3$ is $0.001 \, kg \, h^{-1}$. The rate of consumption of $H_2$ under the same conditions is ...... $kg \, h^{-1}$.

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

For the reaction $H_2 + I_2 \rightarrow 2HI$,state the correct differential rate law.