Exploring Types of Chemical Reactions: A Comprehensive Guide for Class 10 Science Students

Class – X th, Subject : Science

Chemical reactions and equations

Q.1 The types of chemical reactions given below are-

(1) Pb + CuCl → PbCl + Cu

(2) 2Mg+O→ 2 MgO

(3) ZnO+C→ Zn+CO

(4) CuO+H, Cu + H₂O

(5) CuSO+Zn → ZnSO + Cu

(6) CuSO + Fe → FeSO4 + Cu

(7) AgNO,+KCI → AgCl + KNO,

(8) CaO + H₂O → Ca(OH) + heat

(9) 2FeSO, FeO + SO + SO,

(10) 2Pb(NO₂), 2PbO+4NO2 + O

(11) Na₂SO₄ + BaSO → BaSO + 2NaCl

(12) 2PbO + C2 Pb+ Pb + CO,

(13) FeO,+2Al→ AlO + 2Fe

(14) MnO2 + 4HCl → MnCl2 + 2H₂O + CI

(15) CaCO, CaO + CO

Types of Chemical Reactions Explained in English:

Here’s an explanation of the types of chemical reactions given in your question:

(1) Pb + CuCl → PbCl + Cu (Single Displacement):

• Lead (Pb) replaces copper (Cu) in copper chloride (CuCl) to form lead chloride (PbCl) and pure copper (Cu).

(2) 2Mg + O → 2MgO (Combination):

• Two magnesium atoms (Mg) combine with one oxygen atom (O) to form two magnesium oxide molecules (MgO).

(3) ZnO + C → Zn + CO (Redox):

• Zinc oxide (ZnO) loses oxygen to carbon (C), forming zinc metal (Zn) and carbon monoxide (CO). This involves oxidation (ZnO loses oxygen) and reduction (C gains oxygen).

(4) CuO + H2 → Cu + H2O (Redox):

• Copper oxide (CuO) loses oxygen to hydrogen gas (H2), forming copper metal (Cu) and water (H2O). Again, oxidation and reduction occur.

(5) CuSO4 + Zn → ZnSO4 + Cu (Single Displacement):

• Zinc (Zn) displaces copper (Cu) in copper sulfate (CuSO4), forming zinc sulfate (ZnSO4) and pure copper (Cu).

(6) CuSO4 + Fe → FeSO4 + Cu (Single Displacement):

• Similar to above, iron (Fe) replaces copper (Cu) in copper sulfate (CuSO4) to form iron sulfate (FeSO4) and copper (Cu).

(7) AgNO3 + KCl → AgCl + KNO3 (Double Displacement):

• Silver nitrate (AgNO3) and potassium chloride (KCl) exchange ions, forming silver chloride (AgCl) and potassium nitrate (KNO3).

(8) CaO + H2O → Ca(OH)2 + heat (Combination):

• Calcium oxide (CaO) reacts with water (H2O) to form calcium hydroxide (Ca(OH)2), releasing heat.

(9) 2FeSO4 → FeO + SO2 + SO3 (Decomposition):

• Iron sulfate (FeSO4) breaks down into iron oxide (FeO), sulfur dioxide (SO2), and sulfur trioxide (SO3).

(10) 2Pb(NO2)2 → 2PbO + 4NO2 + O2 (Decomposition):

• Lead nitrite (Pb(NO2)2) decomposes into lead oxide (PbO), nitrogen dioxide (NO2), and oxygen (O2).

(11) Na2SO4 + BaCl2 → BaSO4 + 2NaCl (Double Displacement):

• Sodium sulfate (Na2SO4) and barium chloride (BaCl2) exchange ions, forming barium sulfate (BaSO4) and sodium chloride (NaCl).

(12) 2PbO + C → Pb + PbO2 + CO2 (Redox):

• Carbon (C) reduces one lead oxide molecule (PbO) to lead metal (Pb), while oxidizing another to lead dioxide (PbO2). Carbon dioxide (CO2) is also formed.

(13) Fe2O3 + 2Al → Al2O3 + 2Fe (Redox):

• Aluminum (Al) reduces iron oxide (Fe2O3) to iron metal (Fe), forming aluminum oxide (Al2O3). Oxidation and reduction occur simultaneously.

(14) MnO2 + 4HCl → MnCl2 + 2H2O + Cl2 (Redox):

• Manganese dioxide (MnO2) loses oxygen to hydrochloric acid (HCl), forming manganese chloride (MnCl2), water (H2O), and chlorine gas (Cl2).

(15) CaCO3 → CaO + CO2 (Decomposition):

• Calcium carbonate (CaCO3) breaks down into calcium oxide (CaO) and carbon dioxide (CO2).