In the reaction $2 N_{2}O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the ratio of the rate of formation of $NO_{2(g)}$ to the rate of formation of $O_{2(g)}$ is:

Nitric oxide reacts with $H_2$ according to the reaction: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_2 O_{(g)}$. Identify the correct relation for the rate of disappearance of reactants and the rate of appearance of products.

Consider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) is:

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

For the reaction $2A \rightarrow 3C + D$, the rate of reaction is represented by:

For a reaction $\frac{1}{2} A \rightarrow 2 B$,the rate of disappearance of $A$ is related to the rate of appearance of $B$ by the expression: