Matching Chemical Processes with Reaction Types

Let's analyze each chemical process listed and identify the type of chemical reaction involved. Understanding the different types of chemical reactions is fundamental in chemistry.

Here are the processes and their corresponding reaction types:

A. Electrolysis of Water

Electrolysis of water is the process of splitting water ($\text{H}_2\text{O}$) into oxygen ($\text{O}_2$) and hydrogen gas ($\text{H}_2$) using an electric current. A single compound (water) breaks down into simpler substances. This type of reaction where a compound breaks down into two or more simpler substances is called a decomposition reaction.

The chemical equation for the electrolysis of water is:

$\text{2H}_2\text{O(l)} \xrightarrow{\text{Electricity}} \text{2H}_2\text{(g)} + \text{O}_2\text{(g)}$

Therefore, Electrolysis of water matches with Decomposition reaction (3).

B. Burning of Coal

Burning of coal is essentially the reaction of carbon (the main component of coal) with oxygen from the air to produce carbon dioxide. In this process, two or more reactants (carbon and oxygen) combine to form a single product (carbon dioxide). This type of reaction is known as a combination reaction.

The chemical equation for the burning of coal (carbon) is:

$\text{C(s)} + \text{O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)}$

Therefore, Burning of coal matches with Combination reaction (2).

C. Iron Nail Immersed in Copper Sulphate Solution

When an iron nail is placed in a copper sulphate ($\text{CuSO}_4$) solution, iron ($\text{Fe}$) is more reactive than copper ($\text{Cu}$). Iron displaces copper from the copper sulphate solution, forming iron(II) sulphate ($\text{FeSO}_4$) and depositing copper. This reaction where a more reactive element displaces a less reactive element from its compound is a displacement reaction.

The chemical equation for the reaction is:

$\text{Fe(s)} + \text{CuSO}_4\text{(aq)} \rightarrow \text{FeSO}_4\text{(aq)} + \text{Cu(s)}$

Therefore, Iron nail immersed in copper sulphate solution matches with Displacement reaction (4).

D. Addition of Barium Chloride Solution to Aluminium Sulphate Solution

When barium chloride ($\text{BaCl}_2$) solution is added to aluminium sulphate ($\text{Al}_2(\text{SO}_4)_3$) solution, the barium ions ($\text{Ba}^{2+}$) from barium chloride react with sulphate ions ($\text{SO}_4^{2-}$) from aluminium sulphate to form a precipitate of barium sulphate ($\text{BaSO}_4$). Simultaneously, aluminium ions ($\text{Al}^{3+}$) from aluminium sulphate react with chloride ions ($\text{Cl}^-$) from barium chloride to form aluminium chloride ($\text{AlCl}_3$). This reaction involves the exchange of ions between the two reactant compounds. Such a reaction is called a double displacement reaction.

The chemical equation for the reaction is:

$\text{3BaCl}_2\text{(aq)} + \text{Al}_2(\text{SO}_4)_3\text{(aq)} \rightarrow \text{3BaSO}_4\text{(s)} + \text{2AlCl}_3\text{(aq)}$

Therefore, Addition of barium chloride solution to aluminium sulphate solution matches with Double displacement reaction (1).

Summary of Matches

Based on the analysis, we can summarize the matches between List I and List II:

• A. Electrolysis of water $\rightarrow$ 3. Decomposition reaction
• B. Burning of coal $\rightarrow$ 2. Combination reaction
• C. Iron nail immersed in copper sulphate solution $\rightarrow$ 4. Displacement reaction
• D. Addition of barium chloride solution to aluminium sulphate solution $\rightarrow$ 1. Double displacement reaction

This gives us the combination A - 3, B - 2, C - 4, D - 1.

Comparing this derived combination (A - 3, B - 2, C - 4, D - 1) with the provided options, we find that this matches one of the given choices.

Revision Table: Chemical Reaction Types

Additional Information on Chemical Reactions

Chemical reactions are processes that involve the rearrangement of atoms and molecules to form new substances. They are represented by chemical equations, which show the reactants (starting substances) on the left side and the products (substances formed) on the right side.

• Reactants: The substances that undergo change in a chemical reaction.
• Products: The new substances formed as a result of a chemical reaction.
• Chemical equations must be balanced to satisfy the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction.
• Besides the types discussed, other reaction types include redox reactions (involving electron transfer) and acid-base reactions (neutralization).
• Displacement reactions and many combination/decomposition reactions can also be classified as redox reactions. Double displacement reactions typically are not redox reactions unless one of the products decomposes immediately.

Understanding these basic types helps in predicting the products of chemical reactions and analyzing chemical processes occurring in various fields, from industry to biological systems.