For a spontaneous reaction, the free energy change must be negative. , is the enthalpy change during — Metallurgy and Isolation of Elements Chemistry Question

Question

For a spontaneous reaction, the free energy change must be negative. $\Delta G = \Delta H - T\Delta S$, $\Delta H$ is the enthalpy change during the reaction. T is the absolute temperature, and $\Delta S$ is the change in entropy during the reaction. Consider a reaction such as the formation of an oxide $M + O_2 \rightarrow MO$ Dioxygen is used up in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids. Consequently gases have a higher entropy than liquids and solids. In this reaction S (entropy or randomness) decreases, hence $\Delta S$ is negative. Thus, if the temperature is raised then $T\Delta S$ becomes more negative. Since, $T\Delta S$ is substracted in the equation, then $\Delta G$ becomes less negative. Thus, the free energy change increases with the increase in temperature. The free energy changes that occur when one mole of common reactant (in this case dioxygen) is used may be plotted graphically against temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. [SEE DIAGRAM]