The false statement among the following is (1) ΔH for the thermal decomposition process is alway

step 1 The false statement among the following is Delta H for the thermal decomposition process is alwa

The false statement among the following is (1) ΔH for the...

The false statement among the following is (1) $\Delta H$ for the thermal decomposition process is always positive. (2) Bond-breaking cnergy of a molecule is always positive. (3) Conversion of oxygen into ozone is endothermic reaction and hence it is more stable than oxygen. (4) The heat change in a chemical reaction is represented by enthalpy change.

The false statement among the following is
(1) $\Delta H$ for the thermal decomposition process is always positive.
(2) Bond-breaking cnergy of a molecule is always positive.
(3) Conversion of oxygen into ozone is endothermic reaction and hence it is more stable than oxygen.
(4) The heat change in a chemical reaction is represented by enthalpy change.

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Key Concepts

Enthalpy Change

Enthalpy change represents the heat absorbed or released during a chemical reaction at constant pressure. It reflects the energy difference between reactants and products and is a key factor in determining whether a reaction is endothermic (positive enthalpy change) or exothermic (negative enthalpy change).

Thermal Decomposition

Thermal decomposition is a process in which a compound breaks down into simpler substances when heated. These reactions are generally endothermic since energy is required to break chemical bonds, though not every decomposition process strictly follows this pattern without exceptions.

Bond Dissociation Energy

Bond dissociation energy is the energy required to break a specific chemical bond in a molecule. This energy is always positive, as breaking any chemical bond necessitates an input of energy to overcome the forces holding the atoms together.

Endothermic and Exothermic Reactions and Their Impact on Stability

Endothermic reactions absorb energy and lead to products that are higher in energy and generally less stable than the reactants, whereas exothermic reactions release energy, resulting in more stable products. This distinction is crucial when evaluating claims about relative stability based solely on the enthalpy nature of a reaction.

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