Chemical Reactions and Equations Class 10 Science Notes Maharashtra Board

Chemical Reactions and Equations Class 10 Science Notes Maharashtra State Board

In earlier standards, we have seen how compounds are formed by chemical combinations of elements. We have also learned that the driving force behind the formation of a chemical bond is to attain an electronic configuration with a complete octet. The atoms attain a complete octet by giving, taking, or sharing electrons.

Chemical Reaction

Some of the scientists of the 18th and 19th centuries carried out fundamental experiments on chemical reactions. They proved from their experiments that during chemical reactions composition of the matter changes and that change remains permanent. On the contrary, during physical change, only the state of matter changes and this change is often temporary in nature. Identify physical and chemical changes from the phenomena given in the following table.

Apparatus: Thermometer, evaporating dish, tripod stand, funnel, Bunsen burner, etc.
Chemicals: Lime stone powder, copper sulphate, calcium chloride, potassium chromate, zinc dust, sodium carbonate, phthalic anhydride, etc.
Procedure: Carry out the activities 1 to 5 as given below. Read and record the temperatures in the activities 2 to 4.

1. Take a spoonful of limestone powder in an evaporating dish. Heat it strongly on a high blue flame.
2. Add zinc (Zn) dust into the copper sulphate (CuSO₄) solution.
3. Add potassium chromate (K₂CrO₄) solution to barium sulphate (BaSO₄) solution.
4. Add sodium carbonate (Na₂CO₃) solution to the calcium chloride (CaCl₂) solution.
5. Take phthalic anhydride in the evaporating dish.

Close the end of the stem of a funnel with a cotton plug. Keep this funnel inverted on the evaporating dish. Heat the evaporating dish on a tripod stand slowly on a low flame. What did you observe in the funnel during heating? Record the observation of all the activities. What did you find? Complete the following observation table with reference to the activities 1 to 5.

A physical change takes place due to change in the parameters such as temperature, pressure. Often a physical change in reversible. The composition of matter remains the same in a physical change. For example, ice is transformed into water on heating and water is transformed into ice on cooling. On the contrary, if the composition of matter changes during a process then it is called a chemical change. When we call a particular process or phenomenon as a chemical change, some chemical reactions are taking place in the concerned matter.

A chemical reaction is a process in which some substances undergo bond breaking and are transformed into new substances by formation of new bonds. The substances taking part in chemical reaction are called reactants, whereas the substances formed as a result of a chemical reaction by formation of new bonds are called products. For example, formation of carbon dioxide gas by combustion of coal in air is a chemical reaction. In this reaction coal (carbon) and oxygen (from air) are the reactants while carbon dioxide is the product. A chemical reaction is represented by writing a chemical equation.

Chemical Equations

Let us first look at a chemical reaction. In the activity 2, a colourless solution of zinc sulphate (ZnSO₄) is formed on addition of zinc dust to the blue solution of copper sulphate (CuSO₄). This chemical reaction can be written in brief as follows.
Aqueous Solution of Copper Sulphate + Zinc Dust → Aqueous Solution of Zinc Sulphate + Copper ……….(1)
This simple way of representating a chemical reaction in words is called a ‘Word Equation’. A word equation can be written in a further condensed form by using chemical formulae as follows.
CuSO₄ + Zn → ZnSO₄ + Cu ………….. (2)
The representation of a chemical reaction in a condensed form using chemical formulae is called as the chemical equation. In the above equation coper sulphate (CuSO₄) and zinc(Zn) are the reactants. They react with each each other to form copper particles (Cu) and a solution of the colourless zinc sulphate (ZnSO₄) as the products having totally different properties. The ionic bond in the reaction CuSO₄ breaks and the ionic bond in the product ZnSO₄ is formed during the reaction.

Writing a Chemical Equation

Let us now see the conventions followed while writing a chemical equation.
1. In a chemical equation the reactants are written on the left hand side while the products on the right hand side. An arrow heading towards the products is drawn in between them. This arrow indicates the direction of the reaction.

2. If the reactants or products are two or more, they are linked with a plus sign (+) in between them. For example, in the equation (2) a plus sign (+) is drawn in between the reactants CuSO₄ and Zn. Similarly, a plus sign (+) is drawn in between the products ZnSO₄ and Cu.

3. To make the chemical equation more informative the physical states of the reactants are indicated in the equation. Their gaseous, liquid and solid states are indicated by writing the letters (g), (l) and (s), respectively in the brackets. Moreover, if the product is gaseous, instead of (g) it can be indicated by an arrow pointing upwards. If the product formed is insoluble solid, in the form of a precipitate, then instead of (s) it can be indicated by an arrow pointing downwards. When reactants and products are in the form of solution in water, they are said to be present in aqueous solution state. This state is indicated by putting the letters aq in brackets after their formula. Thus, the equation (2) is rewritten as equation (3) shown below.
CuSO₄ (aq) + Zn (s) → ZnSO₄ (aq) + Cu (s) …………….. (3)

4. When heat is to be given from outside to bring about a reaction, it is indicated by the sign ∆ written above the arrow that indicates the direction of the reaction. For example, the reaction in which slaked lime is formed on heating lime stone is written as follows.
CaCO₃ (s) \(\stackrel{\Delta}{\longrightarrow}\) CaO (s) + CO₂ ↑……………… (4)
Similarly, the fact that heat is released during the reaction between the aqueous solution of copper sulphate and zinc dust is indicated as follows.
CuSO₄ (aq) + Zn (s) → ZnSO₄ (aq) + Cu (s) + Heat …………….. (5)

5. It is necessary to fulfil certain conditions like specific temperature, pressure, catalyst, etc, to bring about some reactions. These conditions are indicated below or above the arrow indicating the direction of the reaction. For example, the reaction of a vegetable oil takes place at the temperature of 60°C with hydrogen gas in presence of the Ni catalyst and is written as follows.
Vegetable Oil (l) + H₂ (g) \(\underset{\text { Ni Catalyst }}{\stackrel{60^{\circ} \mathrm{C}}{\longrightarrow}}\) Vanaspathi Ghee (s) ………….(6)

6. Special information or names of reactants/ products are written below their formulae. For example, copper on reaction with concentrated nitric acid gives reddish coloured poisonous nitrogen di oxide gas.
Cu(s) + 4HNO₃ (aq) (Concentrated) → Cu(NO₃)₂ (aq) + 2NO₂ (g) + 2H₂O (l) ………..(7)
However, on reaction with dilute nitric acid, the product formed is nitric oxide gas.
3Cu(s) + 8HNO₃ (aq) (dilute) → 3Cu(NO₃)₂ (aq) + 2NO (g) + 4H₂O (l) ………..(8)

Apparatus: Test tube, conical flask, balance, etc.
Chemicals: Sodium chloride and silver nitrate.
Procedure:

1. Take sodium chloride solution in a conical flask and silver nitrate solution in a test tube.
2. Tie a thread to the test tube and insert it carefully into the conical flask. Make the conical flask air tight by fitting a rubber cork.
3. Weigh the conical flask with the help of a balance.
4. Now tilt the conical flask and mix the solution present in the test tube with the solution in the conical flask.
5. Weigh the conical flask again.

Which changes did you find? Did any insoluble substance form? Was there any change in the weight?
A word equation is written for the above activity as shown below.
Silver nitrate + Sodium chloride → Silver chloride + Sodium nitrate
The above word equation is represented by the following chemical equation.
AgNO₃ (aq) + NaCl (aq) → AgCl↓ (white) + NaNO₃ (aq) …….. (9)

Balancing a Chemical Equation

Complete the table aside on the basis of the equation (9).

Element	Reactants (Left Side)	Products (Right Side)
	Number of Atoms	Number of Atoms
Ag
N
O
Na
Cl

It is seen that the number of atoms of the elements in the reactants in this equation is the same as the number of atoms of those elements in the products. Such an equation is called a ‘balanced equation’. If the number of atoms of each element is not the same on the two sides of an equation, it is called an ‘unbalanced equation’.

In any reaction, the total mass of each of the elements in the reactants is same as the total mass of each of the respective elements in the products. This is in accordance with the law of conservation of mass that you studied in the previous standard.

Steps in Balancing a Chemical Reaction

A chemical equation is balanced step by step. A trial and error method is used for this purpose. Consider the following equation as an example:
Sodium Hydroxide + Sulphuric Acid → Sodium Sulphate + Water

STEP I. Write the chemical equation from the given word equation.
NaOH + H₂SO₄ → Na₂SO₄ + H₂O …………..(10)

STEP II. Check whether the equation (10) is balanced or not by comparing the number of atoms of the various elements present on the two sides of the equation. It is seen that the number of atoms of all the elements on the two sides are not the same. It means that the equation (10) is not balanced.

Element	Reactants (Left Side)	Products (Right Side)
	Number of Atoms	Number of Atoms
Na	1	2
O	5	5
H	3	2
S	1	1

STEP III: It is convenient to start balancing an equation from the compound that contains the maximum number of atoms. Moreover, it is convenient to first consider the element in this compound, which has an unequal number of atoms on the two sides.

Number of Sodium Atoms	In the Reactants (in NaOH)	In the Products (in Na2SO4)
Initially	1	2
To Balance	1 × 2	2

(i) In equation (10), there are two components Na₂SO₄ and H₂SO₄, which contain the maximum number that is seven atoms each. Any one of them can be selected. Select the compound Na₂SO₄. Further select sodium for balancing as the number of atoms of sodium in this compound is unequal on the two sides. It should be remembered that, the formula of a compound cannot be changed while balancing the number of atoms. It means that, here to make the number of sodium atoms in the reactants as ‘2’ the formula NaOH cannot be changed to Na₂OH. Instead a factor of ‘2’ will have to be applied to NaOH. Write down the resulting equation (10)’ on doing this.
2NaOH + H₂SO₄ → Na₂SO₄ + H₂O …………..(10)’

(ii) Check whether the equation (10)’ is balanced or not. We find that the equation (10)’ is not balanced, as the number of oxygen and hydrogen atoms are unequal on the two sides. First balance the hydrogen number as it requires a smaller factor.

(iii) Apply a factor ‘2’ to the product ‘H2O’ for balancing the equation (10)’. Now write down the resulting equation (10)”.
2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O ……..(10)”

(iv) Check whether the equation (10)” is balanced or not. It is seen that the number of atoms of all the elements are equal on both the sides. It means that the equation (10)” is balanced.

Element	Reactants (Left Side)	Products (Right Side)
	Number of Atoms	Number of Atoms
Na	2	2
O	6	5
H	4	2
S	1	1

Step IV: Write down the final balanced equation again.
2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O ……..(11)

Number of Atoms of Hydrogen	In the Reactants (In NaOH & H2SO4)	In the Products (In H2O)
Initially	4	2
To Balance	4	2 × 2

In this way, a balanced equation is obtained from an unbalanced equation by applying proper factors to the appropriate reactant/product to balance the number of each element in steps. We saw that in chemical reactions reactants get converted into new substances called products. During this, some chemical bonds in the reactants break and some new chemical bonds are formed to transform the reactants into the products. In this chapter, we will be studying the types of reactions in detail.

Types of Chemical Reactions

Chemical reactions are classified into the following four types by the nature and the number of the reactants and the products.

1. Combination Reaction
Apparatus: Test tube, glass rod, beaker, etc.
Chemicals: Hydrochloric acid, ammonia solution, slaked lime, etc.

Activity 1: Take a small amount of hydrochloric acid in a test tube. Heat the test tube. Dip a glass rod in the ammonia solution and hold on the top of the test tube. You will observe a white smoke emanating from the tip of the glass rod.

What must have happened?
Due to heating HCl vapours started coming out from the test tube, and NH₃ gas came out from the solution on the glass rod. The ammonia gas and hydrogen chloride gas reacted to form the salt ammonium chloride in gaseous state first, but immediately due to the condensation process at room temperature it got transformed into the solid state. As a result white smoke was formed. The chemical equation for this is as follows.
NH₃ (g) (Ammonia) + HCl (g) (Hydrogen Chloride) → NH₄Cl (s) (Ammonium Chloride) …………………(12)

Activity 2: Hold a magnesium (Mg) strip in a pair of tongs and ignite. On burning in air a white powder of magnesium oxide is formed. The reaction can be written in the form of equation as shown below.
2Mg + O₂ → 2MgO ……………………….(13)
In this reaction magnesium oxide is formed as the single product by combination of magnesium and oxygen.

Activity 3: Take water in a beaker up to half of its capacity. Add a few pieces of slaked lime (calcium oxide, CaO) to it. Calcium hydroxide (Ca(OH)₂) is formed by combination of calcium oxide and water with generation of large amount of heat.
CaO (Calcium Oxide) + H₂O → Ca(OH)₂ (Calcium Hydroxide) + Heat ………………… (14)
When two or more reactants combine in a reaction to form a single product, it is called a combination reaction.

2. Decomposition Reaction
Apparatus: Evaporating dish, Bunsen burner, etc.
Chemicals: Sugar, calcium carbonate, sulphuric acid, etc.
Procedure: Take some sugar in an evaporating dish and heat it with the help of a Bunsen burner. After some time you will see the formation of a burnt-out black substance. Exactly what must have happened in this activity? In the above activity, a single reactant sugar is divided into two substances (C and H₂O)
C₁₂H₂₂O₁₁ (Sugar) → 12C (Carbon) + 11H₂O ………………….(15)
The reaction in which there is only one reactant giving rise to two or more products is called a decomposition reaction.

Apparatus: Two test tubes, bent tube, rubber cork, burner, etc.
Chemicals: Calcium carbonate, freshly prepared lime water.
Procedure: Take some calcium carbonate in a test tube. Fit a bent tube to this test tube with the help of a rubber cork. Insert the other end of the bent tube in the freshly prepared lime water taken in the other test tube. Heat the powdered calcium carbonate in the first test tube strongly. The lime water will turn milky.

We saw in the above activity that calcium carbonate undergoes a decomposition reaction and the carbon dioxide gas formed turns the lime water milky (Eq. 16). The second product of the reaction, the calcium oxide powder, remains behind in the first test tube. Similarly, in another reaction (Eq. 17) hydrogen peroxide naturally undergoes slow decomposition into water and oxygen.
CaCO₃ (s) \(\stackrel{\Delta}{\longrightarrow}\) CaO (s) + CO₂ ↑…….. (16)
2H₂O₂ (l) → 2H₂O (l) + O₂ ↑……. (17)
(16) and (17) both are decomposition reactions.

We have studied in the previous standard that water decomposes into hydrogen and oxygen gases by passing an electric current through acidulated water. This decomposition takes place using electrical energy. Therefore it is called electrolysis.
2H₂O (l) → 2H₂ ↑ + O₂ ↑……..(18)
The chemical reaction in which two or more products are formed from a single reactant is called ‘‘Decomposition reaction”. Many degradation processes take place in the nature surrounding us. Organic waste is decomposed by microorganisms and as a result, manure and biogas are formed. Biogas is used as a fuel.

3. Displacement Reaction
We saw at the beginning of this chapter that on adding zinc dust to blue coloured copper sulphate solution, a colourless solution of zinc sulphate is formed and heat is generated. See the equation (3) for this reaction. From that we learnt that the Zn²⁺ ions formed from Zn atoms take the place of Cu²⁺ ions in copper sulphate, and Cu atoms, formed from Cu²⁺ ion come out. It means that Zn displaces Cu from CuSO₄. The reaction in which the place of the ion of a less reactive element in a compound is taken by another more reactive element by formation of its own ions, is called displacement reaction.

4. Double Displacement Reaction
We have seen in equation (9) that a white precipitate of silver chloride is formed by an exchange of silver and sodium ions present in the reactants. The reaction in which the ions in the reactants are exchanged to form a precipitate is called a double displacement reaction.

Endothermic and Exothermic Processes and Reaction:
Heat is absorbed and given away in various processes and reactions. Accordingly, processes and reactions are classified as ‘Endothermic or Exothermic’.

Endothermic and Exothermic Processes
The heat from outside is absorbed during some physical changes. For example, (i) melting of ice (ii) dissolution of potassium nitrate in water. Therefore, these are ‘Endothermic processes.’

On the other hand, heat is given away during some physical changes. For example, (i) formation of ice from water, (ii) dissolution of sodium hydroxide in water. Therefore these are ‘Exothermic processes.’ In the process of dilution of concentrated sulphuric acid with water, very large amount of heat is liberated. As a result, water gets evaporated instantaneously, if it is poured in to the concentrated sulphuric acid, which may cause an accident. To avoid this, required amount of water is taken in a glass container and small quantity of concentrated sulphuric acid at a time is added with stirring. Therefore, only a small amount of heat is liberated at a time.

To carry out Endothermic and Exothermic Processes
Apparatus: Two plastic bottles, measuring cylinder, thermometer etc.

Chemicals: Potassium nitrate, sodium hydroxide, water etc.
(Sodium hydroxide being corrosive, handle it carefully in presence of Teacher.)

Procedure: Take 100 ml water in each of the two plastic bottles. Plastic being insulator of heat, the dissipation of heat can be prevented. Note the temperature of water in the bottles. Put 5 g potassium nitrate (KNO₃) in the bottle and shake well. Note the temperature of the solution formed. Put 5 g sodium hydroxide (NaOH) in the other bottle. Shake the bottle well. Note the temperature. In the first bottle the process of dissolution of potassium nitrate took place while in the second bottle the process of dissolution of sodium hydroxide took place. As per your observation which one is exothermic process and which is an endothermic process?

During the process of the dissolution of KNO₃ in water, heat from the surroundings is absorbed and therefore the temperature of the resulting solution is less. The process in which heat is absorbed from the outside, is called endothermic process. When the solid NaOH is dissolved in water heat is given out, and therefore the temperature increases. The processes in which heat is given out are called exothermic processes.

Endothermic and Exothermic Reactions
There is an exchange of heat in chemical reactions as well. Accordingly some chemical reactions are exothermic while some other are endothermic. During exothermic chemical reactions heat is given away when reactants are transformed into the products, while during endothermic chemical reactions heat is either absorbed from the surroundings or has to be supplied continuously from outside. For example,
CaCO₃ (s) + Heat → CaO (s) + CO₂ (g) (Endothermic Reaction)
CaO (s) + H₂O (l) → Ca(OH)₂ (aq) + Heat (Exothermic Reaction)

Rate of Chemical Reaction

Take into account the time required for following processes. Classify them into two groups and give titles to the groups.

1. Cooking gas starts burning on ignition.
2. Iron article undergoes rusting.
3. Errosion of rocks takes place to form soil.
4. Alcohol is formed on mixing yeast in glucose solution under proper condition.
5. Effervescence is formed on adding baking soda into a test tube containing dilute acid.
6. A white precipitate is formed on adding dilute sulphuric acid to barium chloride solution.

It can be seen from the above examples that some reactions are completed in short time, that is, occur rapidly, while some other require long time for completion, that is, occur slowly. It means that the rate of different reactions is different.

The same reaction occurs at a different rate on changing the conditions. For example, during winter long time is required for setting milk into curd, while at the higher temperature during summer, the rate of setting of milk increases and the curd is formed early. Now let us see the factors which decide the rate of a chemical reaction.

Factors Affecting the Rate of a Chemical Reaction

Nature of the Reactants
Let us see the reaction of the metals aluminium (Al) and zinc (Zn) with dilute hydrochloric acid. On reaction of both Al and Zn with dilute hydrochloric acid H₂ gas is liberated and water soluble salts of these metals are formed. However, the reaction of aluminium metal takes place faster as compared to zinc metal. The nature of the metal is responsible for this difference. Al is more reactive than Zn. Therefore the rate of reaction of Al with hydrochloric acid is higher than that of Zn. Nature or reactivity of reactants influences the rate of a chemical reaction. (We are going to learn more about the reactivity of metals in the chapter on Metallurgy.)

Size of the Particles of Reactants
Apparatus: Two test tubes, balance, measuring cylinder, etc.
Chemicals: Pieces of Shahabad tile, powder of Shahabad tile, dilute HCl etc.
Procedure: Take pieces and powder of shahabad tile in equal weights in two test tubes. Add 10 ml dilute HCl in each of the test tubes. Observe whether effervescence of CO₂ is formed at a faster or slower speed. You must have found in the above activity that the CO₂ effervescence is formed slowely with the pieces of Shahabad tile while at a faster speed with the powder. The above observation indicates that the rate of a reaction depends upon the size of the particles of the reactants taking part in the reaction. Smaller the size of the reactant particles, higher is the rate of the reaction.

Concentration of the Reactants
Let us consider the reaction of dilute and concerntrated hydrochloric acid with CaCO₃ powder. Dilute HCl reacts slowly with CaCO₃ and thereby CaCO₃ disappears slowly and CO₂ also liberates slowly. On the other hand the reaction with concentrated HCl takes place rapidly and CaCO₃ disappears fast. Concentrated acid reacts faster than dilute acid, which means that rate of a reaction is proportional to the concentration of reactants.

Temperature of the Reaction
While studying decomposition reaction, you have carried out decomposition of lime stone. In this activity, the lime water does not turn milky before heating the lime stone; because of the zero rate of reaction. From this it is learnt that the rate of a reaction increases on increasing the temperature.

Catalyst
On heating potassium chlorate (KClO3) decomposes slowly.
2KClO₃ \(\stackrel{\Delta}{\longrightarrow}\) 2KCl + 3O₂ …….(19)
The rate of the above reaction neither increases by reducing the particle size nor by increasing the reaction temperature. However, KClO3 decomposes rapidly in presence of manganese dioxide (MnO₂) to liberate O₂ gas. No chemical change takes place in MnO₂ in this reaction.

“The substance in whose presence the rate of a chemical reaction changes, without causing any chemical change to it, is called a catalyst.” The decomposition of hydrogen peroxide into water and oxygen takes place slowly at room temperature (Eq. 17). However, the same reaction occurs at a faster rate on adding manganese dioxide (MnO₂) powder in it.

1. One or more chemical reactions take place during every chemical change.
2. Some chemical reactions occur at fast speed whereas some occur at slow speed.
3. Strong acid and strong base react instantaneously.
4. In our body, enzymes increase the rate of physiological reactions.
5. Perishable foodstuff gets preserved longer in a refrigerator. The rate of decomposition of foodstuff gets lowered due to low temperature, and its freshness is maintained.
6. Vegetables cook quickly on oil rather than on water.
7. The chemical reactions are profitable in the chemical factories if their rate is fast.
8. The rate of chemical reaction is important from environmental point of view as well.
9. The ozone layer in the earth’s atmosphere protects the life on earth from the ultraviolet radiation of the sun.
10. The process of depletion or maintenance of this layer depends upon the rate of production or destruction of ozone molecules.

Oxidation and Reduction

Many types of substances give reactions called oxidation and reduction. Let us learn more about these reactions.
2Mg + O₂ → 2MgO ……….(20)
C + O₂ → CO₂ ……….(21)
MgH₂ → Mg + H₂ …….(22)
CH₃ – CH₃ → CH₂ = CH₂ ……(23)
In reactions (20) and (21) a reactant combines with oxygen, whereas in (22) and (23) hydrogas is removed from the reactant. All these are examples of the oxidation reaction. The chemical reaction in which a reactant combines with oxygen or loses hydrogen to form the product is called oxidation reaction.

Some oxidation reactions are brought about by use of specific chemical substances. For example,
CH₃ – CH₂ – OH \(\frac{[\mathrm{O}]}{\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7 / \mathrm{H}_2 \mathrm{SO}_4}\) CH₃ – COOH (Acetic Acid) …….. (24)
Here the acidic potassium dichromate makes oxygen available for the oxidation of the reactant ethyl alcohol. Such chemical subastances which bring about an oxidation reaction by making oxygen available are called oxidants or oxidizing agents.

A variety of oxidants are used to bring about a controlled oxidation. K₂Cr₂O₇/H₂SO₄, KMnO₄/H₂SO₄ are the commonly used chemical oxidants. Hydrogen Peroxide (H₂O₂) is used as a mild oxidant. Ozone (O₃) is also a chemical oxidant. Nascent oxygen is generated by chemical oxidants and it is used for the oxidation reaction.
O₃ → O₂ + [O]
H₂O₂ → H₂O + [O]
K₂Cr₂O₇ + 4H₂SO₄ → K₂SO₄ + Cr₂(SO₄)₃ + 4H₂O + 3[O]
2KMnO₄ + 3H₂SO₄ → K₂SO₄ + 2MnSO₄ + 3H₂O + 5[O]
Nascent oxygen is a state prior to the formation of the O2 molecule. It is the reactive form of oxygen and is represented by writing the symbol as [O].

We have seen just now that potassium permanganate is a chemical oxidant. Now have a look at the following reaction.
2KMnO₄ + 10FeSO₄ + 8H₂SO₄ → K₂SO₄ + 2MnSO₄ + 5Fe₂(SO₄)₃ + 8H₂O …….. (25)
Which compound is oxidised by KMnO₄ in presence of acid in this reaction? Of course FeSO₄. Here FeSO₄ is transformed into Fe₂(SO₄)₃. Let us now see, how this conversion is an oxidation reaction.
2FeSO₄ → Fe₂(SO₄)₃
Ionic reaction, \(\mathrm{Fe}^{2+}+\mathrm{SO}_4^{2-} \rightarrow 2 \mathrm{Fe}^{3+}+3 \mathrm{SO}_4^{2-}\)
The net change taking place in the above conversion is shown by the net ionic reaction as shown below.
Net ionic reaction, Fe²⁺ (Ferrous) → Fe³⁺ (Ferric)
This net ionic reaction represents the oxidation brought about by KMnO₄. When ferric ion is formed from ferrous ion the positive charge is increased by one unit. While this happens the ferrous ion loses one electron. From this, we understand a new definition of oxidation, which is “oxidation means losing one or more electrons.”

The chemical reactions in which reactants gain hydrogen are called ‘reduction’ reactions. Similarly, the reaction in which a reactant loses oxygen to form the product is also called reduction reaction. The substance that brings about reduction is called a reductant, or a reducing agent. When hydrogen gas is passed over black copper oxide a reddish coloured layer of copper is formed. When the positive charge on an atom or an ion increases or the negative charge on them decreases it is called oxidation, and when the positive charge decreases or the negative charge increases it is called reduction.
CuO + H₂ → Cu + H₂O ………..(26)

Which is the Reductant in this Reaction? And which Reactant has undergone Reduction?
In this reaction an oxygen atom goes away from CuO (copper oxide), which means that reduction of copper oxide takes place, whereas hydrogen molecule takes up oxygen atom and water (H₂O) is formed meaning, oxidation of hydrogen takes place. Thus oxidation and reduction reactions occur simultaneously. The reductant is oxidized by the oxidant and the oxidant is reduced by the reductant. Due to this characteristics of the reduction and oxidation reactions, a single term ‘redox reaction’ is used in place of the two terms.
Redox Reaction = Reduction + Oxidation

When the positive charge on an atom or an ion increases or the negative charge on them decreases it is called oxidation, and when the positive charge decreases or the negative charge increases it is called reduction.

A redox reaction takes place during cellular respiration. Here the molecule of the enzyme called cytochrome C oxidase helps the transport of electron to bring about this reaction.

Corrosion
Apparatus: Four test tubes, four small iron nails, rubber cork, etc.
Chemicals: Anhydrous calcium chloride, oil, boiled water, etc.
Procedure: Place four test tubes on a test tube stand. Take some boiled water in one test tube and put an oil layer on it. Take some salt water in the second test tube. Let there be only air in the third test tube. Take some anhyrous calcium chloride in the fourth test tube. Place a small iron nail in every test tube. Close the fourth test tube with a rubber cork. Let all the four test tubes remain un attended for a few days.

Observe all the four test tubes after a few days. What did you find? Which test tubes had the nails as before? Both water and air are necessary for rusting. The rusting process takes place rapidly in presence of a salt. Have you seen the effect of redox reaction in your everyday life? The new vehicles look shiny, on the contrary old vehicles look dull. A certain type of reddish coloured solid layer collects on their metallic surface. This layer is called ‘rust’. Its chemical formula is Fe₂O₃ . X H₂O.

The rust on iron does not form by a simple reaction of oxygen with iron surface. The rust is formed by an electrochemical reaction. Different regions on the surface of iron become anode and cathode.
1. Fe is oxidised to Fe²⁺ in the anode region.
Fe (s) → Fe²⁺ (aq) + 2e^–
2. O₂ is reduced to form water in the cathode region.
O₂ (g) + 4H⁺ (aq) + 4e^– → 2H₂O (l)
When Fe²⁺ ions migrate from the anode region they react with water and further get oxidised to form Fe³⁺ ions.
A redish coloured hydrated oxide is formed from Fe³⁺ ions. It is called rust. It collects on the surface.
2Fe³⁺ (aq) + 4H₂O (l) → Fe₂O₃ . H₂O (s) + 6H⁺ (aq) ……….. (29)
Due to various components of atmosphere, oxidation of metals takes place, consequently resulting in their damage. This is called ‘corrosion’. Iron rusts and a redish coloured layer is collected on it. This is corrosion of iron. Corrosion is a very serious problem.

Rancidity
When we use old, left over cooking oil for making food stuff, it is found to have foul odour called rancidity. If food is cooked in such oil, its taste also changes. When oil or ghee is left aside for a long time or fried food is left aside for a long time it undergoes air oxidation and becomes rancid. Rancidity in the food stuff cooked in oil or ghee is prevented by using antioxidants. The process of oxidation reaction of food stuff can also be slowed down by storing it in air tight container.

Well-organized Maharashtra State Board Class 10 Science Notes Chemical Reactions and Equations can aid in exam preparation and quick revision.