NH2OH - co za związek?

KNO2-----temp--->KO + NO

KNO2-----temp--->KO + NO

KNO2-----temp--->KO + NO

- 2KNO3 --> K2O + N2O + 2O2

5.4.23.1 KNO2
No solid-phase transitions have been reported. The salt begins to decompose noticeably at 410°C.
The first step in the decomposition sequence is probably87,88
2 KNO2 = K2O + NO2 +NO
Between 410 and 460°C the NO produced reacts with KNO2:
KNO2 + 2 NO = 2 KNO3 + N2
The NO2 produced in the first reaction reacts further:
K2O + 2 NO2 = KNO2 + KNO3
KNO2 + NO2 = KNO3 + NO
Which reactions are favored depend largely on the atmospheric composition. For example, in an
inert atmosphere which removes the gaseous products the first reaction will predominate. Otherwise,
since KNO3 is stable in this temperature range and N2 is unreactive, the net result of the above
reactions is the production of KNO3 and N2. In an oxygen atmosphere, particularly in the temperature
range 550 to 600°C, the reaction KNO2 + 1/2 O2 = KNO3 goes to completion. In the range
650 to 750°C, KNO3 becomes increasingly unstable and the reaction attains equilibrium. Above
800°C the reaction 2 KNO2 = K2O + N2 + 3/2 O2 goes to completion.87–89 These results are consistent
with endothermic peaks observed by differential scanning calorimetry.90


5.4.23.2 KNO3
The phase transitions are fairly complicated and have been discussed by several authors.91–93 In
addition to the stable low-temperature orthorhombic form II which transforms at 401 K to the
rhombohedral I, there exists a metastable form III which can be obtained by cooling I to 396 K;
III then transforms to II on further cooling to 386 K.
KNO3 melts without decomposition to a liquid which is stable in air to at least 803 K.94 When
heated in air, it begins to decompose near 923 K.95 Between 823 and 1023 K the quasi-equilibrium
KNO3 = KNO2 + 1/2 O2 is set up.89,95,96 The activation energy for the forward reaction is 274 kJ.
If the O2 is removed, KNO2 decomposes, various oxides of nitrogen are produced, and the reaction
is more complicated (see discussion under KNO2). As pointed out above, the two salts tend to
interconvert over a limited temperature range. Above the melting points this leads to a solution
containing both salts. For some specified oxygen partial pressure, e.g., air, the solution composition
is then a unique function of temperature if equilibrium is established. In the range 823 to 1023 K
the equilibrium has been studied by several authors.89,95,96 All these results have been summarized
by Kramer, Munir, and Volponi90 and are consistent with their DSC results.
Densities are listed in Tables 5.54 and 5.55, transitions in Table 5.56 and thermodynamic data
in Tables 5.57 to 5.61.