The reaction between nitrogen and oxygen is given below: 2 N2 (g) + O2 (g) 2 N2O (g) We therefore know that which of the following reactions can also occur? 2 N2O (g) 2 N2 (g) + O2 (g) N2 (g) + 2 O2 (g) 2 NO2 (g) 2 NO2 (g) N2 (g) + 2 O2 (g) None of the Above

a) 2N₂O (g) → 2N₂ (g) + O₂ (g)

Explanation:

Arrange the equations in the proper way for better understanding.

The reaction between nitrogen and oxygen is given below:

2N₂ (g) + O₂ (g) → 2N₂O (g)

We therefore know that which of the following reactions can also occur?

a) 2N₂O (g) → 2N₂ (g) + O₂ (g) b) N₂ (g) + 2O₂ (g) → 2NO₂ (g) c) 2NO₂ (g) → N₂ (g) + 2O₂ (g) d) None of the Above

Solution

Notice that the first equation, a) 2N₂O (g) → 2N₂ (g) + O₂ (g), is the reverse of the original equation, 2N₂ (g) + O₂ (g) → 2N₂O (g).

The reactions in gaseous phase are reversible reactions that can be driven to one or other direction by modifying the conditions of temperature or pressure.

Thus, the equilibrium equation would be:

2N₂ (g) + O₂ (g) ⇄ 2N₂O (g)

Which shows that both the forward and the reverse reactions occur.

Whether one or the other are favored would depend on the temperature and pressure: high temperatures would favor the reaction that consumes more heat (the endothermic reaction) and high pressures would favor the reaction that consumes more moles.

Thus, by knowing that one of the reactions can occur you can conclude that the reverse reaction can also occur.