2N2O5->4NO2+O2,d[N2O5]/dt=k1[N2O5],d[NO2]/dt=k2[N2O5]andd[O2]/dt=k3[N2O5],the relation betweenk1,k2and k3 is what?
To determine the relation between k1, k2, and k3 in the given chemical reaction, we can analyze the stoichiometry of the reaction and the conservation of matter.
The balanced equation you provided is:
2N2O5 -> 4NO2 + O2
Based on this, we can write the rate law expressions for the given reactants and products:
Rate of disappearance of N2O5: -1/2(d[N2O5]/dt) = k1[N2O5]
Rate of appearance of NO2: (d[NO2]/dt) = k2[N2O5]
Rate of appearance of O2: (d[O2]/dt) = k3[N2O5]
From the stoichiometry, we can infer that the rate of disappearance of N2O5 is half the rate of the appearance of NO2 or the rate of appearance of O2.
Thus, we can write the relationship between the rate constants as:
k1 = 2k2 = 2k3
Therefore, the relation between k1, k2, and k3 is that k1 is equal to 2 times k2 and 2 times k3.