Editing Sucrose (section)

===Thermal and oxidative degradation===
Sucrose does not melt at high temperatures. Instead, it decomposes at {{convert|186|°C}} to form [[caramel]]. Like other [[carbohydrate]]s, it combusts to [[carbon dioxide]] and water by the simplified equation:

{{chem2|C12H22O11 + 12 O2 → 12 CO2 + 11 H2O}}

Mixing sucrose with the oxidizer [[potassium nitrate]] produces the fuel known as [[rocket candy]] that is used to propel amateur rocket motors.<ref>{{cite web |url=https://www.nakka-rocketry.net/sucrose.html |first=Richard |last=Nakka| website=Experimental Rocketry |title=Potassium Nitrate/Sucrose Propellant (KNSU) |access-date=2015-11-19 |url-status=live |archive-url=https://web.archive.org/web/20151026075559/https://www.nakka-rocketry.net/sucrose.html |archive-date=2015-10-26}}</ref>

{{chem2|C12H22O11 + 6 KNO3 -> 9 CO + 3 N2 + 11 H2O + 3 K2CO3}}

This reaction is somewhat simplified though. Some of the carbon does get fully oxidized to carbon dioxide, and other reactions, such as the [[water-gas shift reaction]] also take place. A more accurate theoretical equation is:

{{chem2|C12H22O11 + 6.288 KNO3 -> 3.796 CO2 + 5.205 CO + 7.794 H2O + 3.065 H2 + 3.143 N2 + 2.988 K2CO3 + 0.274 KOH}}<ref>{{cite web |url=https://www.nakka-rocketry.net/succhem.html |first=Richard |last=Nakka |website=Experimental Rocketry|title=KN-Sucrose (KNSU) Propellant Chemistry and Performance Characteristics |access-date=2014-08-21 |url-status=live |archive-url=https://web.archive.org/web/20141118052432/https://www.nakka-rocketry.net/succhem.html |archive-date=2014-11-18}}</ref>

Sucrose burns with [[chloric acid]], formed by the reaction of [[hydrochloric acid]] and [[potassium chlorate]]:

{{chem2|8 HClO3 + C12H22O11 -> 11 H2O + 12 CO2 + 8 HCl}}

Sucrose can be dehydrated with concentrated [[sulfuric acid]] to form a black, [[carbon]]-rich solid, as indicated in the following idealized equation:

{{chem2|H2SO4 (catalyst) + C12H22O11 -> 12 C + 11 H2O + heat (and some H2O + SO3 as a result of the heat).}}

The formula for sucrose's decomposition can be represented as a two-step reaction: the first simplified reaction is dehydration of sucrose to pure carbon and water, and then carbon is oxidised to {{chem2|CO2}} by {{chem2|O2}} from air.

{{chem2|C12H22O11 + heat -> 12 C + 11 H2O}}

{{chem2|12 C + 12 O2 -> 12 CO2}}
<div style="float:right;clear:right;margin-left:0.5em;">
{| class="wikitable" style="text-align:center"
|+ Solubility of sucrose in water vs. temperature
! T (°C) !! S (g/dL)
|-
| 50 || 259
|-
| 55 || 273
|-
| 60 || 289
|-
| 65 || 306
|-
| 70 || 325
|-
| 75 || 346
|-
| 80 || 369
|-
| 85 || 394
|-
| 90 || 420
|}
</div>