Question

The formation ½ A2 + 2 B2 + C --> CAB4 has an enthalpy of formation of -104 kJ and a change in entropy of -60.8 J/K at 30 °C. What is the free energy and spontaneity of the reaction?​

Answer 1

Answer:

-82.0 kJ, spontaneous

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Answer 2

Answer:

Concept:

The change in the enthalpy of a chemical reaction that takes place at constant pressure is known as the Heat of Reaction (also known as the Enthalpy of Reaction). It is a thermodynamic unit of measurement that can be used to determine how much energy is released or created per mole during a reaction.

A spontaneous reaction is one that favors the creation of products under the reaction's current conditions.

Explanation:

An illustration of this is a roaring bonfire.

- A fire is exothermic, which implies that when heat is discharged into the environment, the energy of the system decreases. - Because carbon dioxide and water vapor make up the majority of the fire's byproducts, the entropy of the system rises throughout most combustion reactions.

- Because of this loss in energy and rise in entropy, combustion reactions take place spontaneously.

Enthalpy change and entropy change are mathematically combined to form the free energy change of a process.

Given:

The formation ½ A2 + 2 B2 + C --> CAB4

Enthalpy of formation of -104 kJ

At 30 °C.

Find:

What is the free energy and spontaneity of the reaction

Solution:

G = H-T S

by definition, so

$\begin{aligned}&\Delta G=\Delta H-T^{*} \Delta S \\&\Delta G=(-104)-(30+273)^{*}(-60.8)=-104000-(-18422)=-85578 \mathrm{~J}\end{aligned}$

Since $\Delta G < 0$ this is favoring products, therefore it is a spontaneous reaction.

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