SODIUM SUPEROXIDE NaO2

Properties of sodium superoxide NaO2:

The orange-yellow, when heated decomposes without melting. Ion has the structure of the (Na +) (O2-). Reacts with water, acids, mono and dioxide of carbon. A strong oxidizer.


Obtaining sodium superoxide:

Na2O2 + O2 = 2NaO2 (450—500° C, pressure).

O2 + 2Na = Na2O2 (burning in air, the impurity of Na2O)

O2 + Na2O2 = 2 Na2O (400° C, pressure).


Reactions with sodium superoxide:

Na2O (-O2, 100-270°C) → Na2O2( -O2, 400-675°) C, vacuum

2 Na2O + H2O (cold) = NaOH + NaHO2(solution) + O2↑

2 NaHO2 (solution) →(time) 2 NaOH + O2↑ (normal temp.).

4 Na2O + 2 H2O (hot) = 4 NaOH + 302↑.

2 Na2O + 2 HCl (diluted, cold) = 2NaCl + H2O2 + O2↑.

4 Na2O + 2CO2 = 2Na2CO3 + 3O2 (normal temp.).

2 Na2O + CO = Na2CO3 + O2 (100° С).

4 Na2O + З С (graphite) = 2 Na2CO3 + CO2 (100° С).

Na2O + Аl (powder) = NaAlO2 (100° С).
 

Did you know?

The only elements that are liquid at room temperature are bromine and mercury. However, you can melt gallium by holding a lump in the warmth of your hand.