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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 1.80 mol/min at a particular moment, what is the rate of appearance of no2 at that moment?

Respuesta :

meerkat18
The chemical reaction is

2 N₂O₅ (g) → 4 NO₂ (g) + O₂ (g)

In order to know the yield of Nitrogen Dioxide (NO₂) from the Dinitrogen Pentoxide, you have to know the stoichiometric coefficients of the balanced reaction. The balancing of the reaction occurs because of the concept of the Law of Definite Proportions. The number of an element in the reaction must be equal in both sides. From the reaction, we can deduce that in every 2 moles of N₂O₅, 4 moles of NO₂ is produced. Therefore,

1.8 mol NO₂/min * 4 mol NO₂/2 mol  N₂O₅ = 3.6

Thus, 3.6 moles of NO₂ is produced every minute.
pstnonsonjoku

The rate of disappearance of NO2 is -3.6 mol/min.

What is rate of reaction?

The term rate of reaction refers to how quickly or slowly a reaction proceeds. The reaction in question here is 2 N2O5(g) → 4NO2(g) + O2(g).

The question lets us know that the rate of disappearance of N2O5 is 1.80 mol/min. The rate of appearance of NO2 is; d[NO2]/dt = -4/2 (1.80 mol/min) = -3.6 mol/min

Learn more about rate of reaction: https://brainly.com/question/17960050

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