Final answer:
The rate of appearance of NO2 when the rate of disappearance of N2O5 is 1.80 mol/min is 3.60 mol/min based on the stoichiometry of the reaction.
Step-by-step explanation:
The decomposition of dinitrogen pentoxide (N2O5) is described by the chemical equation 2 N2O5(g) → 4 NO2(g) + O2(g). The rate of disappearance of N2O5 is given as 1.80 mol/min. According to the stoichiometry of the reaction, 4 moles of NO2 are produced for every 2 moles of N2O5 that decompose. Therefore, the rate of appearance of NO2 at that moment would be twice the rate of the disappearance of N2O5, which is 1.80 mol/min * 2 = 3.60 mol/min.