Consider the decomposition of liquid benzene, C₆H₆(l), to gaseous acetylene, C₂H₂(g): C₆H₆(l) → 3 C2H₂(g) ΔH = +630 kJ (d) If C₆H₆(g) were consumed instead of C₆H₆(l), would you expect the magnitude of ΔH to increase, decrease, or stay the same? Explain.

Key Concepts

Enthalpy Change (ΔH)

Enthalpy change (ΔH) is a measure of the heat content of a system at constant pressure. It indicates whether a reaction is exothermic (releases heat, ΔH < 0) or endothermic (absorbs heat, ΔH > 0). In this case, the positive ΔH of +630 kJ signifies that the decomposition of liquid benzene into gaseous acetylene is an endothermic process, requiring energy input.

Phase Changes and Energy

The phase of a substance significantly affects its energy content. Transitioning from a liquid to a gas requires energy to overcome intermolecular forces, which is reflected in the enthalpy change. If benzene is in the gaseous state, it has already absorbed energy to vaporize, potentially altering the overall energy dynamics of the reaction compared to starting with liquid benzene.

Reaction Pathway and Thermodynamics

The thermodynamic properties of a reaction can vary based on the initial and final states of the reactants. The pathway taken during a reaction, including the states of matter involved, can influence the total energy change. If gaseous benzene is consumed instead of liquid, the energy required for the reaction may differ, potentially leading to a different ΔH value, depending on the energy already present in the gaseous state.