calculate how many moles of NO2 form when each of the following completely reacts. 2N2O5 (g) →4NO2 (g) + O2 (g) Part A 1.0 mol N2O5 Express your answer using two significant figures. nothing mol m o l Request Answer Part B 5.4 mol N2O5 Express your answer using two significant figures.

Part A: 2.0 mol.

Part B: 10.8 mol.

Explanation:

For the balanced reaction:

2N₂O₅ (g) → 4NO₂ (g) + O₂ (g),

It is clear that 2 mol of N₂O₅ (g) dissociate to 4 mol of NO₂ (g) and 1 mol O₂ (g).

Part A 1.0 mol N₂O₅:

Using cross multiplication:

2 mol of N₂O₅ (g) produces → 4 mol of NO₂ (g), from stichiometry.

1 mol of N₂O₅ (g) produces →? mol of NO₂ (g),

∴ The no. of moles of NO₂ produced = (1 mol) (4 mol) / (2 mol) = 2.0 mol.

Part B 5.4 mol N₂O₅:

Using cross multiplication:

2 mol of N₂O₅ (g) produces → 4 mol of NO₂ (g), from stichiometry.

5.4 mol of N₂O₅ (g) produces →? mol of NO₂ (g),

∴ The no. of moles of NO₂ produced = (5.4 mol) (4 mol) / (2 mol) = 10.8 mol.