POTASSIUM SUPEROXIDE KO2

Properties potassium superoxide KO2:

The orange-yellow, decomposes when heated, melts under excess pressure. It has the ionic structure (K +) (O2-). Reacts with water, acids, mono-and carbon dioxide, ozone, potassium, ammonia. It is a strong oxidizing agent.


Obtaining potassium superoxide KO2:

K + O2(air) = KO2 (combustion, impurity K2O2).


Chemical reactions with potassium superoxide KO2:

KO2 -O2→(290°C, vacuum) K2O2 -O2 → (530°C) K2O.

2KO2 + H2O = КОН + KHO2 (solution) + O2↑ (0°C),

2KHO2 (solution) → time → 2KОН + O2↑ (normal temp.).

4KO2 + 2H2O (burning) = 4KОН + 3O2↑.

2KO2 + 2HСl (diluted, cold) = 2KСl + H2O2 + O2↑.

2KO2 + H2SO4 (anhydrous) = K2SO4 + O3↑ + H2O (normal temp.).

KO2 + O3 = KO3 + O2 (until 0°C, in the liquid CCl2F2).

2KO2 + S = K2SO4 (130—140°C),

2KO2 + SO2 = K2SO4 + O2 (100°C).

4KO2 + 3C (graphite) = 2K2CO3 + CO2 (30°C).

4KO2 + 2CO2 (humidity) = 2 K2CO3 + 3O2 (normal temp.).

2KO2 + СO = K2CO3 + O2 (50°C).

2KO2 + 2 NO2 = 2KNO3 + O2 (70°C).

KO2 + 3K = 2 K2O (700°C, pressure).

2KO2 + 2NH3 → time → 2KOH + N2 + 2H2O (normal temp.).


 

Did you know?

Hydrogen is the most abundant element in the universe, while oxygen is the most abundant element in the earth's atmosphere, crust, and oceans (about 49.5%).