Classify the following reactions into different types, giving a reason
(a) $ C a O(s)+S i O_{2}(g) \quad \longrightarrow \quad C a S i O_{3}(s) $(b) $ K O H(a q)+H C l(a q) \quad \longrightarrow \quad K C l(a q)+H_{2} O(l) $(c) $ \mathrm{Cu}(\mathrm{s})+2 \mathrm{AgNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Cu}\left(\mathrm{NO}_{2}\right)_{2}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s}) $(d) $ B a C O_{3}(s) \stackrel{\text { heat }}{\longrightarrow} B a O(s)+C O_{2}(g) $
(a) CaO (s) + SiO2 (g) → CaSiO3 (s)
This is a Synthesis or Combination Reaction: A combination reaction (also known as a synthesis reaction) is a reaction where two or more elements or compounds (reactants) combine to form a single compound (product). Such reactions are represented by an equation of the following form: X + Y → XY.
CaO(s) + SiO2(g) ⟶ CaSiO3(s)
(b) KOH(aq) + HCl(aq) ⟶ KCl(aq) + H2O(l)
This is a Double Displacement Reaction: A double-replacement reaction is a reaction in which the cations and anions of two ionic compounds exchange places to form two new compounds.
The general form of a double-replacement (also called double-displacement) reaction is AB + CD → AD + BC.
KOH(aq) + HCl(aq) ⟶ KCl(aq) + H2O(l)
(c) Cu (s) + 2AgNO3 (aq) ⟶ Cu(NO3)2 (aq) + 2Ag (s)
This is a Displacement Reaction: Displacement reaction is a chemical reaction in which a more reactive element displaces a less reactive element from its compound. Both metals and non-metals take part in displacement reactions.
(d) BaCO3 (s) ⟶ BaO(s) + CO2 (g)
This is a Decomposition Reaction: Decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more elements or new compounds. These reactions often involve an energy source such as heat, light, or electricity that breaks apart the bonds of compound.
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