Answer:
[tex]r=\frac{r(NO_{2})}{2} =\frac{r(O_{2})}{1/2}=\frac{r(N_{2}O_{5})}{1}[/tex]
Explanation:
Let us consider the reaction:
2 NO₂ + 1/2 O₂ ⇄ N₂O₅
The rate of formation of a substance is equal to the change in concentration of the product divided the change in time:
[tex]r(N_{2}O_{5})=\frac{\Delta [N_{2}O_{5}] }{\Delta t}[/tex]
The rate of disappearance of a reactant is equal to to the change in concentration of the reactant divided the change in time, with a negative sign so that the rate is always a positive variable.
[tex]r(NO_{2})=-\frac{\Delta[NO_{2}] }{\Delta t}[/tex]
[tex]r(O_{2})=-\frac{\Delta[O_{2}] }{\Delta t}[/tex]
The rate of the reaction is equal to the rate of any substance divided its stoichiometric coefficient. In this way, we can relate these expressions:
[tex]r=\frac{r(NO_{2})}{2} =\frac{r(O_{2})}{1/2}=\frac{r(N_{2}O_{5})}{1}[/tex]
