give 4 type of chemical reaction
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4 types of chemical reactions:
1. Synthesis / Direct Combustion
These chemical reactions occur where two or more substances react together to form just one product. Synthesis reactions are usually exothermic, though they might sometimes require an addition of heat energy to start off.
Examples: In the presence of heat iron (II) and sulfur is such an example.
Fe + S →→ FeS
One the reaction takes off in the presence of heat, it then continues exothermally. Formation of Aluminium Iodide is quite a spontaneous reaction and takes place in the presence of a few drops of water.
Al + 3I2 →→ 2 AlI3
However, there is one synthesis reaction which is endothermic, which is photosynthesis. This is a type of photochemical reaction. Carbon dioxide and water react to form glucose in the presence of sunlight and chlorophyll.
6CO2 + 6H2O →→ C6H12O6 + 6O2
Combustion is a type of synthesis reaction which is basically an exothermic reaction which takes place in the presence of oxygen as one of the reactants. Substances such as methane (natural gas) undergo combustion readily to give out a large amount of energy.
CH4 + 2O2 →→ CO2 + 2H2O
2. Decomposition reaction
Decomposition reactions have just one reactant which breaks up to from two or more simpler products. Usually, decomposition reactions are endothermic as they require an input of heat and so such decomposition reactions are known as thermal decomposition reactions.
Examples:
The heating of mercury (II) oxide yield oxygen and mercury
2HgO →→ 2Hg + O2
Lime (calcium oxide) is manufacture from limestone (calcium carbonate) for making cement by the process of decomposition.
CaCO3 →→ CaO + CO2
Decomposition reactions can take off even in the presence of light as in the case of silver chloride.
2AgCl →→ 2Ag + Cl2
AgCl is a white solid and turns grey on the formation of silver metal.
3. Single Displacement
Such types of chemical reactions occur when a more reactive element displaces a less reactive one from a solution its compounds.
Examples:
Zinc is a more reactive element/ metal than copper. So, Copper is displaced from copper (II) sulfate solution.
Zn + CuSO4 →→ ZnSO4 + Cu
Similar is the case when Magnesium is placed in hydrochloric acid. Hydrogen being less reactive than magnesium is displaced.
Mg + 2HCl →→ MgCl2 + H2
4. Double Displacement
Double displacement chemical reactions involve the exchange of ions between two salts in aqueous solutions. Neutralization and precipitation reactions are types of double displacement reactions.
In neutralization reactions, the reaction occurs between a base and an acid. The acidity (of the acid) is destroyed thus ‘neutralizing’ its effect and producing a salt and water.
Example:
H2SO4 + CuO →→ CuSO4 + H2O
Precipitation reaction involves the formation of a precipitate or an insoluble product when ions in solution combine. This reaction occurs when two solutions are mixed or when a gas is bubbled through a solution.
Example:
Pb(NO3)2 + 2KI →→ PbI2 + 2KNO3
1. Synthesis / Direct Combustion
These chemical reactions occur where two or more substances react together to form just one product. Synthesis reactions are usually exothermic, though they might sometimes require an addition of heat energy to start off.
Examples: In the presence of heat iron (II) and sulfur is such an example.
Fe + S →→ FeS
One the reaction takes off in the presence of heat, it then continues exothermally. Formation of Aluminium Iodide is quite a spontaneous reaction and takes place in the presence of a few drops of water.
Al + 3I2 →→ 2 AlI3
However, there is one synthesis reaction which is endothermic, which is photosynthesis. This is a type of photochemical reaction. Carbon dioxide and water react to form glucose in the presence of sunlight and chlorophyll.
6CO2 + 6H2O →→ C6H12O6 + 6O2
Combustion is a type of synthesis reaction which is basically an exothermic reaction which takes place in the presence of oxygen as one of the reactants. Substances such as methane (natural gas) undergo combustion readily to give out a large amount of energy.
CH4 + 2O2 →→ CO2 + 2H2O
2. Decomposition reaction
Decomposition reactions have just one reactant which breaks up to from two or more simpler products. Usually, decomposition reactions are endothermic as they require an input of heat and so such decomposition reactions are known as thermal decomposition reactions.
Examples:
The heating of mercury (II) oxide yield oxygen and mercury
2HgO →→ 2Hg + O2
Lime (calcium oxide) is manufacture from limestone (calcium carbonate) for making cement by the process of decomposition.
CaCO3 →→ CaO + CO2
Decomposition reactions can take off even in the presence of light as in the case of silver chloride.
2AgCl →→ 2Ag + Cl2
AgCl is a white solid and turns grey on the formation of silver metal.
3. Single Displacement
Such types of chemical reactions occur when a more reactive element displaces a less reactive one from a solution its compounds.
Examples:
Zinc is a more reactive element/ metal than copper. So, Copper is displaced from copper (II) sulfate solution.
Zn + CuSO4 →→ ZnSO4 + Cu
Similar is the case when Magnesium is placed in hydrochloric acid. Hydrogen being less reactive than magnesium is displaced.
Mg + 2HCl →→ MgCl2 + H2
4. Double Displacement
Double displacement chemical reactions involve the exchange of ions between two salts in aqueous solutions. Neutralization and precipitation reactions are types of double displacement reactions.
In neutralization reactions, the reaction occurs between a base and an acid. The acidity (of the acid) is destroyed thus ‘neutralizing’ its effect and producing a salt and water.
Example:
H2SO4 + CuO →→ CuSO4 + H2O
Precipitation reaction involves the formation of a precipitate or an insoluble product when ions in solution combine. This reaction occurs when two solutions are mixed or when a gas is bubbled through a solution.
Example:
Pb(NO3)2 + 2KI →→ PbI2 + 2KNO3
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there are four basic chemical reactions types: 1)synthesis or direct reaction
2)decomposition
3) single displacement
4)double displacement.
examples are,
1)Fe + S →→ FeS
2)2HgO →→ 2Hg + O2
3)Zn + CuSO4 →→ ZnSO4 + Cu
4)H2SO4 + CuO →→ CuSO4 + H2O
hope this help u buddy
2)decomposition
3) single displacement
4)double displacement.
examples are,
1)Fe + S →→ FeS
2)2HgO →→ 2Hg + O2
3)Zn + CuSO4 →→ ZnSO4 + Cu
4)H2SO4 + CuO →→ CuSO4 + H2O
hope this help u buddy
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