Calculate the free energy change for this reaction at 25 °C. Is the reaction spontaneous? (Assume that all reactants and products are in their standard states.) 2 Ca(s) + O₂( g) → 2 CaO(s) ΔH°_rxn = -1269.8 kJ; ΔS°_rxn = -364.6 J/K

검증된 단계별 안내

Identify the formula for calculating the Gibbs free energy change: \( \Delta G^\circ = \Delta H^\circ - T \Delta S^\circ \).

Convert the temperature from Celsius to Kelvin: \( T = 25 + 273.15 = 298.15 \text{ K} \).

Ensure that the units for \( \Delta S^\circ \) are consistent with \( \Delta H^\circ \). Convert \( \Delta S^\circ \) from J/K to kJ/K by dividing by 1000: \( \Delta S^\circ = -364.6 \text{ J/K} = -0.3646 \text{ kJ/K} \).

Substitute the values into the Gibbs free energy equation: \( \Delta G^\circ = -1269.8 \text{ kJ} - (298.15 \text{ K} \times -0.3646 \text{ kJ/K}) \).

Determine if the reaction is spontaneous by checking the sign of \( \Delta G^\circ \). If \( \Delta G^\circ < 0 \), the reaction is spontaneous.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Gibbs Free Energy

Gibbs Free Energy (G) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. The change in Gibbs Free Energy (ΔG) for a reaction can be calculated using the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. A negative ΔG indicates that a reaction is spontaneous under the given conditions.

Standard State Conditions

Standard state conditions refer to a set of specific conditions used to measure the properties of substances, typically defined as 1 bar of pressure and a specified temperature, usually 25 °C (298 K). Under these conditions, the standard enthalpy (ΔH°) and standard entropy (ΔS°) values are determined for reactants and products. These values are essential for calculating the Gibbs Free Energy change for reactions, as they provide a reference point for the thermodynamic properties.

Spontaneity of Reactions

The spontaneity of a reaction refers to whether a reaction can occur without external intervention. A reaction is considered spontaneous if it leads to a decrease in free energy (ΔG < 0). Factors influencing spontaneity include enthalpy (ΔH) and entropy (ΔS) changes; a reaction can be spontaneous at certain temperatures even if it is endothermic (positive ΔH) if the entropy increase (positive ΔS) is sufficiently large to make ΔG negative.

Calculate the free energy change for this reaction at 25 °C. Is the reaction spontaneous? (Assume that all reactants and products are in their standard states.) 2 Ca(s) + O2( g) → 2 CaO(s) ΔH°rxn = -1269.8 kJ; ΔS°rxn = -364.6 J/K