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------------------------------------------------ Consider the reduction of gaseous sulfur trioxide, SO3(g), to form sulfur dioxide:

SO3(g) → SO2(g) + \(\frac{1}{2}\) O2(g)

ΔH = 98.3 kJ

(a) What is the enthalpy change for the reverse reaction?

ΔH_reverse = ___ kJ/mol.

The enthalpy change for the reverse reaction in the given chemical process is -98.3 kJ/mol as it is the opposite of the enthalpy change for the forward reaction. This indicates that the reverse reaction is endothermic. Enthalpy change is a concept in Thermodynamics, a part of Physical Chemistry.

Explanation:

The enthalpy change for the reverse reaction of the reduction of gaseous sulfur trioxide, SO3(g), to form sulfur dioxide, SO2(g), and oxygen, 1/2 O2(g), is the opposite of the enthalpy change for the forward reaction.

In the case of your question, the enthalpy change for the forward reaction is 98.3 kJ. Hence, the enthalpy change for the reverse reaction (Hreverse) would be -98.3 kJ/mol, meaning the reaction is endothermic in nature.

Enthalpy change, also known as heat of reaction, relates to the amount of energy absorbed or released by a chemical reaction. This term is typically used in the field of Thermodynamics, part of Physical Chemistry. An understanding of these principles is useful in predicting how chemical reactions will proceed under different conditions.

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