Q.Write the rate law for the following reactions.

The rate law $\text{Rate}=k[A]^m[B]^n$ links rate to concentration through the rate constant k and the orders m, n -- exponents that MUST be measured experimentally and can never be assumed equal to the balanced equation's own stoichiometric coefficients. The overall order is $m+n$. Proof this matters: for $2NO(g)+O_2(g)\rightarrow2NO_2(g)$, experiment shows the reaction is SECOND order in NO (not first, despite NO's coefficient being 2 -- a coincidental match, not a rule) and first order in $O_2$, giving overall order 3. …