In a reaction `2N_(2)O_(5) to 4NO_(2)+O_(2)` the rate can be expressed as
(i) `-(d[N_(2)O_(5)])/(dt) =k_(1)[N_(2)O_(5)]`
(ii) `(d[NO_(2)])/(dt) =k-(2)[N_(2)O_(5)]`
(iii) `(d[O_(2)])/(dt) =k_(3)[N_(2)O_(5)]`
How are `k_(1),k_(2) and k_(3) `related ?

Explanation

To find the relationship between the rate constants \( k_1 \), \( k_2 \), and \( k_3 \) for the reaction

\[ 2N_{2}O_{5} \rightarrow 4NO_{2} + O_{2} \]

we start by expressing the rates of change of concentrations based on the stoichiometry of the reaction.

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