Why is burning of natural gas classified as an exothermic reaction?

Question

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The correct answer is Option C: Because heat is produced in this reaction. Burning of natural gas is classified as an exothermic reaction because it releases a significant amount of energy into the surroundings in the form of heat. In any chemical reaction where the total energy of the products is less than the total energy of the reactants, the excess energy is liberated.

Step-by-Step Solution & Concepts:
Burning of natural gas is classified as an exothermic reaction because it releases a significant amount of energy into the surroundings in the form of heat. In any chemical reaction where the total energy of the products is less than the total energy of the reactants, the excess energy is liberated.

Working Principle: Natural gas consists primarily of methane ($CH_4$). During combustion, methane reacts with oxygen ($O_2$) to form carbon dioxide ($CO_2$) and water ($H_2O$). The chemical bonds in the reactants are broken and new, more stable bonds are formed in the products, resulting in the net release of energy as thermal energy.

Key Formulas: $CH_4(g) + 2O_2(g) ightarrow CO_2(g) + 2H_2O(l) + 	ext{Heat}$; $\Delta H

Key Points: Exothermic reactions release thermal energy.; Combustion is the most common type of exothermic reaction.; The products ($CO_2$ and $H_2O$) are more stable than the reactants ($CH_4$ and $O_2$).

Advantages: Efficient source of thermal energy for cooking and industrial processes.

Disadvantages: Produces greenhouse gases like carbon dioxide which contribute to global warming.

Applications: Used in gas stoves for domestic cooking.; Used in gas turbines for power generation.

Additional Info: Standard Enthalpy of combustion for Methane is approximately $-890 	ext{ kJ/mol}$.. Option B is incorrect because it describes an endothermic reaction, which absorbs heat from the environment.

Answer: C is correct — Because heat is produced in this reaction

Exam Tip: Always remember that breaking bonds requires energy (endothermic), but forming new, stronger bonds releases more energy than what was consumed, leading to the overall exothermic nature of combustion.

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Option A: Because it involves a change in state

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Option B: Because it absorbs heat

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Option D: Because it produces light

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Option E: None of the above

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