`2NO + H_(2) to N_(2)O + H_(2)O` , The reaction , follows third order kinetics.
Write (a) rate law and (b) units of rate constant.
What happens to the rate if the volume of vessel is reduce to one - half at constnat temperature ?

Explanation

(a)Rate law is given as, rate ` = k[NO]^(2) [H_(2)]`
(b) Units of rate constant ` = L^(2) mol^(-2)s^(-1)`
If volume of the vessel in halved , concentration of each reactant is doubled . The rate will be
Rate `= k[2NO]^(2) [2H_(2)] = 8k[NO]^(2) [H_(2)]`
Rate will be 8 times more than the original rate of the reaction .