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Fireworks! - Redox Reaction
Transcript of Fireworks! - Redox Reaction
January Campbell: Block 1
all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between species
SiCl4 + 2 H2O = 4 HCl + SiO2
NH4NO3(s) = N2O(g) + 2 H2O(l)
2 KNO3 + S + 3 C = 3 CO2 + K2S + N2
Produce the oxygen to burn the mixture inside the firework
Typically nitrates, chlorates or perchlorates
Most commonly used are nitrates
What is a Firework?
- a device that contains gunpowder, and other combustible material that causes a beautiful explosion when ignited
Redox in Fireworks
made from a metal ion and a nitrate ion
only give up 1/3 of their oxygen
metal ion and a chlorate ion
give up all their oxygen, causing a more spectacular reaction
have more oxygen but are less likely to explode if you drop them
metal ion and perchlorate poytomic ion
burn the oxygen produced by the oxidizers to produce hot gasses
Two examples are Sulfur and Charcoal
They reacts with oxygen to form Sulfur Dioxide and Carbon Dioxide
Usually two reducing agents are combined to produce a speeding or lowing of the reaction.
Used t control the speed of the reaction - the finer the powder the faster the reacion due to concentration
hold the mixture in a lump (a star)
In a star, two main elements are used that are dampened, rolled, and cut to form the final product that is a firework.
produced by vaporizing zinc chloride
the hydrolysis of silicon chloride