Suppose the reduction of nitric oxide proceeds by the following mechanism:

$1)$ H$2($g$)+2$NO$($g$)----->$N$20($g$)+$ H$20($g$)$ k$1$

$2)$ H$2($g$)+$ N$20($g$)----->$ N$2($g$)+$ H$20($g$)$ k$2$

Suppose also k$1>>$k$2$ That is$,$ the first step is much faster than the second.

a$)$ Write the balanced chemical equation for the overall chemical reaction:

b$)$ Write the experimentally$-$ observable rate law for the Overall chemical reaction.

Note: your answer should not contain the concentrations Of any intermediates.

c$)$ Express the rate constant k for the overall chemical reaction in terms of k$1,$ k$2),$ and $($if necessary$)$ the rate constants k$1$ and k$2$ for the reverse of the two elementary reactions in the mechanism.