Question

For the reaction shown, calculate how many moles of NO2 form when each amount of reactant completely reacts.
2N2O5(g)→4NO2(g)+O2(g)
Part B

5.3 molN2O5 (Express your answer using two significant figures.)

Part C

4.76×103molN2O5 (Express your answer using three significant figures.)

Part D

1.015×10−3molN2O5 (Express your answer using four significant figures.)

Answer 1

Solution :

The reaction is given as :

In the above reaction we can see that, 2 moles of N₂O₅ decomposes to form 4 moles of NO₂ and 1 mole O₂.

Part B :

2 moles of N₂O₅ decomposes to form 4 moles of NO₂

So, 5.3 moles of N₂O₅ will decompose to form = (4/2)5.3 = 10.6 11 moles of NO₂

Therefore, 5.3 moles of N₂O₅ will decompose to form = 11 moles of NO₂

Part C :

2 moles of N₂O₅ decomposes to form 4 moles of NO₂

So, 4.76 10³ moles of N₂O₅ will decompose to form = (4/2) 4.76 10³ = 9.52 10³ moles of NO₂

Therefore, 4.76 10³moles of N₂O₅ will decompose to form = 9.52 10³ moles of NO₂

Part D :

2 moles of N₂O₅ decomposes to form 4 moles of NO₂

So, 1.015 10^-3 moles of N₂O₅ will decompose to form = (4/2) 1.015 10^-3 = 2.03 10^-3 moles of NO₂

Therefore, 1.015 10^-3 moles of N₂O₅ will decompose to form = 2.030 10^-3 ​moles of NO₂