Explain the difference between instantaneous rate of a reaction and average rate of a reaction.

If the rate of disappearance of $N_2O_5$ in the following reaction is $1.2 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$,the rate of production of $NO_2$ in $mol \ L^{-1} \ s^{-1}$ is:
$2N_2O_{5(g)} \longrightarrow 4NO_{2(g)} + O_{2(g)}$

For the reaction $4 NH_3 + 5 O_2 \rightarrow 4 NO + 6 H_2 O$,if the rate of disappearance of $NH_3$ is $3.6 \times 10^{-3} \ M/s$,what is the rate of formation of water?

Give the definition of the following terms:
$(i)$ Rate of Reaction
$(ii)$ Average rate of reaction
$(iii)$ Instantaneous rate

For the reaction $4NH_3 + 5O_2 \to 4NO + 6H_2O$,if the rate of disappearance of $NH_3$ is $3.6 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,what is the rate of formation of $H_2O$?

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 $H_2$?