Question

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g) → 4 NO2(g) + O2(g) If the rate of disappearance of N2O5 is equal to 2.20 mol/min at a particular moment, what is the rate of appearance of NO2 at that moment?

Answer 1

Answer:

$r_{N_2O_5}=4.40mol/min$

Explanation:

Hello,

For the given reaction, the rate of disappearance of nitric oxide (negative as it is a reactant) has the following relationship with the rate of appearance of nitrogen dioxide, in terms of their stoichiometric coefficients:

$-\frac{1}{2} r_{N_2O_5}=\frac{1}{4} r_{NO_2}\\r_{NO_2}=-2r_{N_2O_5}\\r_{N_2O_5}=-2*(-2.20mol/min)\\r_{N_2O_5}=4.40mol/min$

Best regards.