For a certain chemical reaction, ΔH^∘=-35.4 kJ and ΔS^∘=-85.5 J / K . (a) Is the reaction exot

step 1 Starting with option A, the given value for delta H is negative 35 .4 kilojoules. Here we have a

For a certain chemical reaction, ΔH^∘=-35.4 kJ and...

For a certain chemical reaction, $\Delta H^{\circ}=-35.4 \mathrm{~kJ}$ and $\Delta S^{\circ}=-85.5 \mathrm{~J} / \mathrm{K} .$ (a) Is the reaction exothermic or endothermic? (b) Does the reaction lead to an increase or decrease in the randomness or disorder of the system? (c) Calculate $\Delta G^{\circ}$ for the reaction at $298 \mathrm{~K} .(\mathbf{d})$ Is the reaction spontaneous at $298 \mathrm{~K}$ under standard conditions?

For a certain chemical reaction, $\Delta H^{\circ}=-35.4 \mathrm{~kJ}$ and $\Delta S^{\circ}=-85.5 \mathrm{~J} / \mathrm{K} .$ (a) Is the reaction exothermic or endothermic? (b) Does the reaction lead to an increase or decrease in the randomness or disorder of the system?
(c) Calculate $\Delta G^{\circ}$ for the reaction at $298 \mathrm{~K} .(\mathbf{d})$ Is the reaction spontaneous at $298 \mathrm{~K}$ under standard conditions?

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Key Concepts

Gibbs Free Energy (?G)

Gibbs Free Energy is a thermodynamic potential used to predict the spontaneity of a reaction at constant temperature and pressure. It is calculated using the relationship ?G = ?H - T?S. This equation incorporates both the system’s heat change and the change in disorder, thereby providing an overall criterion for spontaneity.

Reaction Spontaneity

A reaction is considered spontaneous if the Gibbs free energy change is negative (?G < 0) under the given conditions. This indicates that the combination of enthalpy, entropy, and temperature effects favors the progress of the reaction, leading to products being formed without the need for external energy input.

Enthalpy (?H)

Enthalpy is a measure of the total heat content of a system. In the context of chemical reactions, a negative enthalpy change indicates that the reaction releases heat to the surroundings, classifying it as exothermic, while a positive enthalpy change indicates that heat is absorbed, classifying it as endothermic.

Entropy (?S)

Entropy quantifies the degree of randomness or disorder in a system. A positive entropy change means the system’s disorder increases as the reaction occurs, whereas a negative entropy change indicates that the disorder decreases, often due to a more ordered arrangement of molecules in the products compared to the reactants.

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