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For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g)+O2(g) Step 1: O3(g)+NO2(g)→NO3(g)+O2(g) slow Step 2: NO3(g)+NO2(g)→N2O5(g) fast View Available Hint(s) For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: Step 1: slow Step 2: fast Rate=k[O3][NO2]2 Rate=k[NO3][NO2] Rate=k[O3][NO2] Rate=k[O3][NO2]2[N2O5][O2]

Respuesta :

Answer: [tex]Rate=k[O_3][NO_2]^2[/tex]

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

[tex]O_3(g)+NO_2(g)\rightarrow NO_3(g)+O_2(g)[/tex]   slow

[tex]NO_3(g)+NO_2(g)\rightarrow N_2O_5(g)[/tex]   fast

To determine the net chemical equation, we will simply add the above two equations, we get:

[tex]O_3(g)+2NO_2(g)\rightarrow N_2O_5(g)+O_2(g)[/tex]

[tex]Rate=k[O_3][NO_2]^2[/tex]

Order with respect to [tex]O_3[/tex] is 1 and Order with respect to [tex]NO_2[/tex] is 2.

Thus the rate law will be:  [tex]Rate=k[O_3][NO_2]^2[/tex]

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