(a)Decomposition reaction: These are the reactions in which a compound breaks down to form two or more elements or new compounds.
These reactions require a source of energy (heat, light or electrical) to proceed.
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Types of decomposition reaction are as follows (based on source of energy):
In the presence of heat (Thermal decomposition reaction):
CaCO3(s)Heat−−→CaO(s)+CO2(g)
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In the presence of sunlight (Photolytic decomposition reaction):
2AgCl(s)Sunlight−−−−−→2Ag(s)+Cl2(g)
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In the presence of electricity (Electrolytic decomposition reaction):
2H2O(l)Electricity−−−−−−→2H2(g)+O2(g)
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(b) In a displacement reaction, a more reactive element displaces a less reactive element from its compound or salt solution.
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For example: CuSO4(aq)+Zn(s)→ZnSO4(aq)+Cu(s)
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In a double displacement reaction, two compounds react by exchanging their ions to form new compounds. It is typically identified by the formation of a product that is a precipitate.
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For example: Na2SO4(aq)+BaCl2(aq)→BaSO4(s)+2NaCl(aq)
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