# The science of fireworks [closed]

1) A simple equation for the reaction: $$\ce{2KNO3 (aq) + C (s) + S (s) -> K2S (s) + N2 (g) + 3 CO2 (g)}$$

The oxidation number of carbon increases from 0 to +4. The oxidation number of nitrogen decreases from +5 to 0. The oxidation number of sulphur decreases from 0 to -2. Are these correct?

2) "Sulfur is used to speed up the reaction and acts like a catalyst in that it increases the rate of reaction. However, unlike a catalyst, it is used up in the reaction." I understand that transition metals are often used as catalysts but why can sulphur act like a catalyst?

3) Potassium Nitrate is a naturally occurring compound. Can we find it easily? Do we often produce it by neutralizing nitric acid with potassium hydroxide?

4) When metals are burnt, metal oxides(some coloured) are formed. Is this the only reason for the beautiful colours of fireworks? When metals are burnt under high temperature, will they turn to plasma state? If so, should the metal ions be responsible for the colours and sparks?

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 It's not entirely clear to me which are the questions you are trying to answer and which portions are your speculations about answers to the questions. Some formatting might help you in that regard. Thank you for at least putting some of your thoughts down, though. – jonsca♦ Feb 17 at 3:50 Each one of these questions is radically different. Could you split it into four separate questions (ask three more questions)? You can cross-link them if you want (or ask us for help with this). I'm closing this for now, ping me to reopen (@Manishearth in a comment), or custom flag this when you want it reopened :) – ManishEarth♦ Feb 17 at 5:24

## closed as not a real question by ManishEarth♦Feb 17 at 5:25

It's difficult to tell what is being asked here. This question is ambiguous, vague, incomplete, overly broad, or rhetorical and cannot be reasonably answered in its current form. For help clarifying this question so that it can be reopened, see the FAQ.