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 1.60 mol/min at a particular moment, what is the rate of appearance of NO2 at that moment?

The answer is 3.20 mol/min.
Please explain the steps I need to take not just solving

Answer 1

you want step by step well here you go

Step-by-step explanation:

To determine the rate of appearance of NO2 at the given moment, we need to use the stoichiometric coefficients of the balanced chemical equation. The balanced equation is: 2 N2O5(g) → 4 NO2(g) + O2(g) 1. The coefficient ratio between N2O5 and NO2 is 2:4, which simplifies to 1:2. This means that for every 1 mol of N2O5 that disappears, 2 mol of NO2 are formed. 2. Given that the rate of disappearance of N2O5 is 1.60 mol/min, we can determine the rate of appearance of NO2 using the coefficient ratio. 3. Since the coefficient ratio is 1:2, the rate of appearance of NO2 will be twice the rate of disappearance of N2O5. 4. Therefore, the rate of appearance of NO2 at that moment is 2 * 1.60 mol/min = 3.20 mol/min. In summary, by using the stoichiometric coefficients of the balanced equation, we find that the rate of appearance of NO2 is 3.20 mol/min when the rate of disappearance of N2O5 is 1.60 mol/min.