Calculate the value of standard molar Gibbs free energy change of chemical reaction at $298 \mathrm{~K}$ using the data given below: Is the chemical reaction exothermic reaction or endothermic? WHY? 4/3Al(s)+O2(g)ष2/3Al2O3 (g) at $298 \mathrm{~K}$

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∻Solution∻ ‖ 1 ⋮ **Identify the given data**: To calculate the standard molar Gibbs free energy change ($\Delta G^\circ$) for the reaction, we need to use the standard Gibbs free energy of formation ($\Delta G_f^\circ$) for the reactants and products. Unfortunately, the OCR model did not provide the $\Delta G_f^\circ$ values for the substances involved in the reaction. Without these values, we cannot calculate $\Delta G^\circ$ for the reaction. ‖ ‖ 2 ⋮ **Determine the nature of the reaction (exothermic or endothermic)**: To determine whether the reaction is exothermic or endothermic, we would typically look at the enthalpy change ($\Delta H$) of the reaction. If $\Delta H$ is negative, the reaction is exothermic; if $\Delta H$ is positive, it is endothermic. However, since the OCR model did not provide the necessary enthalpy data or any indication of heat transfer, we cannot conclusively determine the nature of the reaction from the given information. ‖ ∻Answer∻ ⚹ The standard molar Gibbs free energy change ($\Delta G^\circ$) cannot be calculated without the standard Gibbs free energy of formation values, and the nature of the reaction (exothermic or endothermic) cannot be determined without enthalpy data or heat transfer information. ⚹ ∻Key Concept∻ ⚹ The standard molar Gibbs free energy change of a reaction is calculated using the standard Gibbs free energy of formation for the reactants and products. ⚹ ∻Explanation∻ ⚹ To determine whether a reaction is exothermic or endothermic, we need to know the enthalpy change of the reaction, which indicates whether heat is released or absorbed. ⚹◊What is the formula to calculate the standard molar Gibbs free energy change for a chemical reaction at a given temperature?⍭ Generate me a similar question◊

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