Chemical Reactions And Equations

(i) Hydrogen + Chlorine → Hydrochloric Acid
The above reaction can be written as
H₂ (g) +Cl₂ (g)→ HCl (g)

H₂ (g) + Cl₂ (g) → 2HCl (g)
(ii) Barium chloride + Aluminium sulphate → Barium sulphate + Aluminium chloride
The above equation can be written as
BaCl₂ + Al₂(SO₄)₃ → BaSO₄ + AlCl₃

So, after balancing we get,
3BaCl₂ (s) + Al₂(SO₄)₃ (s) → 3BaSO₄ (s) + 2AlCl₃ (s)
(iii) Na(s) + H₂O (l) → NaOH (aq) + H₂ (g)
Balancing the equation and making the elements equal on both the side, we get:
2Na + 2H₂O → 2NaOH + H₂

(i) Na₂SO₄(aq) + BaCl₂(aq) → BaSO₄(s) + 2NaCl(aq)

(ii) NaOH (aq) + HCl (aq) → NaCl (aq) + H₂O (l)

(i) Substance X is Calcium Oxide whose solution we use in water which is used for white washing.

The formula of substance X is CaO.

(ii) Calcium oxide reacts vigorously with water to produce slaked lime (calcium hydroxide) releasing a large amount of heat.

Electrolysis of Water produces 2 volumes of Hydrogen Gas and 1 Volume of Oxygen gas through which we can conclude that ratio of Hydrogen to Oxygen is 2:1 by Volume in Water. Hence one of test tube has double the amount of gas as compared to other test tube.

• When an iron nail is dipped in copper sulphate solution, then the colour of copper sulphate solution changes because iron displaces copper from copper sulphate solution to form light green solution of iron sulphate.
• Iron is more reactive than copper that's why it is able to displace Copper.
• This reaction is known as displacement reaction
• The reaction involved here is:

**Note: In a double displacement reaction, the positive and the negative ions exchange places and form new products, as shown in the figure given below:

Examples:
1) When Barium Chloride is added to Copper Sulphate Solution, a double displacement reaction takes place resulting in the formation of white precipitate of Barium Sulphate along with Copper Chloride Solution

2) Another Example Double Displacement Reaction is as follow:-

(i)

If a substance gain oxygen during a reaction, it is said to be oxidized. During this reaction, the sodium is gaining oxygen and is being oxidized. Oxygen is getting reduced.

(ii)

During this reaction, copper oxide is losing oxygen and is being reduced. The hydrogen is gaining oxygen and is being oxidized.

Loss of Oxygen is by an element is known Reduction whereas gain of Oxygen by an element is known as Oxidation

Here, lead oxide loses oxygen and is hence reduced. Carbon gains oxygen and hence gets oxidized.

When an element displaces another element from its compound, a displacement reaction occurs.

In this reaction, aluminium displaces the iron from its compound. Thus, this is an example of displacement reaction.

When dilute hydrochloric acid is added to iron fillings, hydrogen gas and iron chloride are produced.

A chemical reaction which has an equal number of atoms of the elements in the reactants and product sides is called a balanced chemical equation.
For example;

Since the number of atoms of each element is the same on both parts of the equation. Hence, it is a balanced chemical equation.

The chemical equation needs to be balanced so that it follows the law of conservation of mass(which states that the 'matter (or atoms) can neither be created nor destroyed in a chemical reaction')

(a) Hydrogen gas combines with nitrogen to form ammonia.
The equation of the above reaction is
H₂ (g) + N₂ (g) → NH₃ (g)
Step 1 - To balance chemical equations, first list the number of atoms of a different type that are present in the chemical equation on both sides –

Step 2 - To start balancing, we take all compound in the reaction and start balancing the reaction

Hence the Balanced Chemical Equation is 3H₂ + N₂ →2NH₃

The following questions are solved similarly.
(b)
Hydrogen sulphide gas burns in air to give water and sulphur dioxide.
The equation of the above chemical change is
H₂S + O₂ → H₂O + SO₂
Step 1 - To balance chemical equations, first list the number of atoms of a different type that are present in the chemical equation on both sides –

Step 2 - To start balancing, we take all compound in the reaction and start balancing the reaction

Hence, the Balanced Chemical Equation is

2H₂S (g) + 3O₂ (g) → 2H₂O (l) + 2SO₂ (g)

The following questions are solved similarly

(c) Barium chloride reacts with aluminium sulphate to give aluminium chloride solution and a precipitate of barium sulphate.

The equation of the above reaction is
BaCl₂ + Al₂(SO₄)₃ (aq) → AlCl₃ (aq) +BaSO₄ (s)
Step 1 - To balance chemical equations, first list the number of atoms of a different type that are present in the chemical equation on both sides –

Step 2 - To start balancing, we take all compound in the reaction and start balancing the reaction.

Thus, we get
3BaCl₂ (aq) + Al₂(SO₄)₃ (aq) → 2AlCl₃ (aq) + 3BaSO₄ (s)

(d) Potassium metal reacts with water to give potassium hydroxide and hydrogen

The equation of the above reaction is
K + H₂O → KOH +H₂
Step 1 - To balance chemical equations, first list the number of atoms of a different type that are present in the chemical equation on both sides –

Step 2 - To start balancing, we take all compound in the reaction and start balancing the reaction

_{Thus, using the above table the balanced chemical equation is}
2K (s) + 2H₂O (l) → 2KOH (aq) + H₂ (g)

(a) Step 1 - To balance chemical equations, first list the number of atoms of different type that are present in the chemical equation on both sides -

HNO₃ + Ca(OH)₂→ Ca(NO₃)₂ + H₂O

Step 2 - To start balancing, we find the compound that has the highest number of atoms. We can see that Ca(NO₃)₂ on the product side has the highest number of atoms. In this compound Oxygen has the highest number of atoms. Lets start with that.

This makes the partially balanced equation -

2HNO₃ + Ca(OH)₂→ Ca(NO₃)₂ + 2H₂O

Step 3 - Now checking for all other elements we note that the number of atoms on both side are same. We can say that the equation is balanced.

(b)NaOH + H₂SO₄→ Na₂SO₄ + H₂O
Step 1 - To balance chemical equations, first list the number of atoms of different type that are present in the chemical equation on both sides –

NaOH + H₂SO₄→ Na₂SO₄ + H₂O

Step 2 - To start balancing, we take any one compound. We will take NaOHon the reactant side in consideration. Let’s start with that.

This makes the partially Balanced Equation as:-

2NaOH + H₂SO₄-> Na₂SO₄ + 2H₂O

Step 3 - Now checking for all other elements we note that the numbers of atoms on both sides are same. We can say that the equation is balanced.

(c) NaCl + AgNO₃→ AgCl + NaNO₃

Step 1 - To balance chemical equations, first list the number of atoms of different type that are present in the chemical equation on both sides –

NaCl + AgNO₃→ AgCl + NaNO₃

_{We can see that the Number of Atoms in LHS and RHS are equal, Hence the equation is already balanced}

(d) BaCl₂ + H₂SO₄→ BaSO₄ + 2HCL
Step 1 - To balance chemical equations, first list the number of atoms of different type that are present in the chemical equation on both sides –
BaCl₂ + H₂SO₄→ BaSO₄ + 2HCL

(a) Ca(OH)₂ + CO₂→ CaC0₃ + H₂0

(b) Zn + 2AgNO₃→ Zn(NO₃)₂ + 2Ag

(c) 2Al + 3CuCl₂→ 2AlCl₃ + 3Cu

(d) BaCl₂ + K₂SO₄→ BaSO₄ + 2KCl

(a) Double displacement reaction (also known as precipitation reaction):-

2KBr (aq) + BaI₂ (aq) → 2KI(q) + BaBr₂ (s)


(b) Decomposition reaction:

(c) Combination reaction:

(d) Displacement reaction:

Exothermic reaction: Reactions in which heat is released along with the formation of products are called exothermic reaction.

For example: Burning of fuel is an example of exothermic reaction. When methane is burnt in the air, heat is produced along with carbon dioxide and water.

Endothermic reaction: Reactions in which energy is absorbed are known as endothermic reactions.

Example: Sliver chloride turns grey in sunlight to form silver metal.

In the process of respiration, the glucose combines with oxygen in the cells of our body to form carbon dioxide and energy is released. That’s why it is considered an exothermic reaction.

In a decomposition reaction, a single substance splits to form two or more simpler substances whereas in combination reaction, two or more substances combine to form a single substance. Hence, decomposition reactions are called the opposite of combination reactions.

(i) Decomposition reaction:

In this reaction, calcium carbonate decomposes into calcium oxide and carbon dioxide on heating. This is an important decomposition reaction used in various industries.

(ii) Combination reaction: Formation of water

In this reaction, two substances hydrogen and oxygen combine to form single substance water, so this is a combination reaction.

We can see from the above examples that a decomposition reaction is opposite of a combination reaction.

(a) In this reaction, calcium carbonate decomposes into calcium oxide and carbon dioxide on heating. This reaction is carried out by heating.

In this reaction, energy is supplied in the form of heat.

(b) Sliver chloride turns grey in sunlight to form silver metal.

In this reaction, energy is supplied in the form of light, i.e. sunlight.

(c) When acidified water is electrolysed, it decomposes to form hydrogen and oxygen:

2H₂0 (I) → 2H₂ (g) + O₂ (g)

In this case, energy is supplied in the form of electricity.

In a displacement reaction, a more reactive element displaces a less reactive element from its solution while in a double displacement reaction, exchange of ions between the reactants takes place to form new products.

(i) Displacement reaction: In this reaction, zinc displaced copper from copper sulphate solution.

(ii) Double displacement reaction:

Displacement reaction is used in the recovery of silver from silver nitrate solution during refining of silver.

Precipitation reaction: Any reaction in which an insoluble solid (called precipitate) is formed, is called a precipitation reaction.

For example: When a solution of silver nitrate is mixed with a solution of sodium chloride, a white precipitate of silver chloride is formed. Hence, it is precipitation reaction.

(a) Oxidation: A chemical reaction in which gain of oxygen or loss of hydrogen takes place.

Example:


Here, magnesium is oxidised to form magnesium oxide.

(b) Reduction: A chemical reaction in which loss of oxygen or gain of hydrogen takes place.

Example:

When zinc oxide is heated with carbon, then zinc metal and carbon monoxide are formed:

In this reaction, Zinc oxide (ZnO) is reduced to zinc by the loss of oxygen.

The unknown element X is copper (Cu). When copper is heated in air, it forms a black coloured compound called copper oxide (CuO). The reaction for above chemical change is given below:

The color of the heated copper powder becomes black when air is passed over it because of its reaction with oxygen i.e Air. When it reacts with oxygen it forms copper oxide which is black in color.

Iron articles are painted to prevent them from rusting. When paint is applied on the surface of iron articles, the contact of air and moisture with iron metals is cut off. Therefore, no rusting takes place.

• The oil and fat present in food items get oxidized in the presence of air forming products having unpleasant smell and taste which turn the food rancid.
• Rancidity makes the food unfit for eating.
• This is why antioxidants are added to foods containing oil and fat to prevent oxidation of food.
• Nitrogen acts as an antioxidant.
• That’s why oil and fat containing food items are flushed with nitrogen to prevent oxidation.
• Thus, the food does not turn rancid and remain good to eat for a longer time.

(b) Rancidity:- Oxidation of Fats and Oils present in food materials by the oxygen present in air resulting in unpleasant smell and taste is called Rancidity. This makes the food not fit for eating.
Example:- Potato Chips that are cooked in oil turn Rancid and give out unpleasant smell and taste if kept exposed for a long time