Explain the following types of chemical reactions giving two examples for each of them:
(a) combination reaction
(b) decomposition reaction
(c) displacement reaction
(d) double displacement reaction

Question

Explain the following types of chemical reactions giving two examples for each of them: (a) combination reaction (b) decomposition reaction (c) displacement reaction (d) double displacement reaction

KnowledgeBoat · Accepted Answer

(a) Combination Reaction — A reaction in which two or more substances combine to form a single substance is called a combination reaction. It is also called a synthesis reaction. Examples: (i) Two elements combine to form a compound. When iron and sulphur (both elements) are heated together they combine to form a compound iron sulphide. Fe (s) + S (s) FeS (s) (ii) An element and a compound can also combine to form a product. Carbon monoxide, a compound, burns in presence of oxygen, an element, to form a single product, carbon dioxide. 2CO (g) + O₂ (g) 2CO₂ (g) (b) Decomposition Reaction — A reaction in which a compound breaks up on heating into two or more simpler substances is called a decomposition reaction. Examples: (i) Calcium carbonate decomposes on strong heating to form two compounds, calcium oxide and carbon dioxide. CaCO₃ (s) CaO (s) + CO₂ (g) (ii) Mercuric oxide when heated decomposes to form mercury and oxygen. 2HgO (s) 2Hg (s) + O₂ (g) (c) Displacement Reaction — A reaction in which a more active element displaces a less active element from a compound is called a displacement reaction. Examples: (i) Zinc is more reactive than copper so it displaces copper from copper sulphate solution to form zinc sulphate. Zn (s) + CuSO₄ (aq) ZnSO₄ (aq) + Cu (s) (ii) Chlorine is more reactive than bromine, so it displaces bromine from potassium bromide solution. 2KBr + Cl₂ 2KCl + Br₂ (d) Double Displacement Reaction — A chemical reaction in which two compounds in their aqueous state exchange their ions or radicals to form new compounds is called a double decomposition reaction. AB + CD CB + AD Here AB and CD are reactants. They exchange their ions to form CB and AD which are the products. Examples: (i) When a solution of silver nitrate is added to a solution of sodium chloride a precipitate of silver chloride is formed. AgNO₃ (aq) + NaCl (aq) NaNO₃ (aq) + AgCl ↓ (ii) When ferrous sulphate solution is added to sodium hydroxide solution, a dirty green precipitate of ferrous hydroxide is formed. FeSO₄ (aq) + 2NaOH (aq) Fe(OH)₂ ↓ + Na₂SO₄ (aq)

Chemistry

Explain the following types of chemical reactions giving two examples for each of them:
(a) combination reaction
(b) decomposition reaction
(c) displacement reaction
(d) double displacement reaction

Chemical Reaction

Related Questions

Define:
(a) Precipitation
(b) Neutralization
(c) Catalyst

How will you obtain?
(a) Magnesium oxide from magnesium.
(b) Silver chloride from silver nitrate.
(c) Nitrogen dioxide from lead nitrate.
(d) Zinc chloride from zinc.
(e) Ammonia from nitrogen.
Also give balanced equations for the reactions.

Chemistry

Explain the following types of chemical reactions giving two examples for each of them:(a) combination reaction(b) decomposition reaction(c) displacement reaction(d) double displacement reaction

Chemical Reaction

Related Questions

Define:(a) Precipitation(b) Neutralization(c) Catalyst

How will you obtain?(a) Magnesium oxide from magnesium.(b) Silver chloride from silver nitrate.(c) Nitrogen dioxide from lead nitrate.(d) Zinc chloride from zinc.(e) Ammonia from nitrogen.Also give balanced equations for the reactions.

Explain the following types of chemical reactions giving two examples for each of them:
(a) combination reaction
(b) decomposition reaction
(c) displacement reaction
(d) double displacement reaction

Define:
(a) Precipitation
(b) Neutralization
(c) Catalyst

How will you obtain?
(a) Magnesium oxide from magnesium.
(b) Silver chloride from silver nitrate.
(c) Nitrogen dioxide from lead nitrate.
(d) Zinc chloride from zinc.
(e) Ammonia from nitrogen.
Also give balanced equations for the reactions.