What is the average rate of reaction when the change in concentration of product is $0.05 \ M$ in $20 \ s$ (in $M \ s^{-1}$)?

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

In a catalytic conversion of $N_2$ to $NH_3$ by Haber's process,the rate of reaction was expressed as change in the concentration of ammonia per time is $40 \times 10^{-3} \ mol \ L^{-1} s^{-1}$. If there are no side reactions,the rate of the reaction as expressed in terms of hydrogen is (in $mol \ L^{-1} s^{-1}$)

If the instantaneous rate of reaction is given as $-\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$,then the reaction is represented as:

In the reaction,$N_{2} + 3H_{2} \longrightarrow 2NH_{3}$,the rate of disappearance of $H_{2}$ is $0.02 \ M/s$. The rate of appearance of $NH_{3}$ is (in $M/s$)

Mention the factors that affect the rate of a chemical reaction.