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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.

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superman1987

Answer:

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.