Question

For the reaction 4.57×10³mol N2O5, calculate how many moles of NO2

form when each amount of reactant completely reacts.

2N2O5(g)→4NO2(g)+O2(g)

Answer 1

To find the moles of NO2 produced from 4.57×10³ mol of N2O5 using the reaction 2N2O5(g) → 4NO2(g) + O2(g), we apply a 1:2 molar ratio, resulting in 9.14×10³ mol of NO2.

Step-by-step explanation:

The problem given revolves around the stoichiometry of a chemical reaction.

In the balanced chemical equation 2N2O5(g) → 4NO2(g) + O2(g), we can determine the number of moles of NO2 produced from a given number of moles of N2O5.

Given 4.57×10³ mol N2O5, we apply the stoichiometry of the reaction to calculate the moles of NO2.

The molar ratio of N2O5 to NO2 in the reaction is 2:4, which simplifies to 1:2.

This means that for each mole of N2O5 that reacts, two moles of NO2 are produced.

Therefore, if 4.57×10³ mol N2O5 completely reacts, we will produce twice that amount in moles of NO2:

moles of NO2 = 4.57×10³ mol N2O5 × (4 mol NO2 / 2 mol N2O5)

= 9.14×10³ mol NO2.