Refer to Ellingham diagram in Q.138. Select the correct...

Refer to Ellingham diagram in Q.138. Select the correct option. For the reduction of $\mathrm{FeO}$ at the temperature at point $R$ is:(1) $\Delta G^{\circ}$ value negative. (2) $\Delta G^{\Theta}$ value for the overall reduction reaction with mixture of a 1 mol of $C$ and 1 mol $\mathrm{O}_{2}$ is positive. (3) $\Delta G^{\ominus}$ value for the overall reduction reaction with 2 $2 \operatorname{mol} \mathrm{C}$ and 1 mol of $\mathrm{O}_{2}$ will be positive. (4) $\Delta G^{\ominus}$ value for the overall reduction reaction with $\mathrm{CO}_{\text {if }}$ zero.

Refer to Ellingham diagram in Q.138. Select the correct option. For the reduction of $\mathrm{FeO}$ at the temperature at point $R$ is:(1) $\Delta G^{\circ}$ value negative.
(2) $\Delta G^{\Theta}$ value for the overall reduction reaction with mixture of a 1 mol of $C$ and 1 mol $\mathrm{O}_{2}$ is positive.
(3) $\Delta G^{\ominus}$ value for the overall reduction reaction with 2 $2 \operatorname{mol} \mathrm{C}$ and 1 mol of $\mathrm{O}_{2}$ will be positive.
(4) $\Delta G^{\ominus}$ value for the overall reduction reaction with $\mathrm{CO}_{\text {if }}$ zero.

Key Concepts

Ellingham Diagram

An Ellingham diagram is a graphical representation that plots the standard Gibbs free energy change (?G°) for various oxidation reactions as a function of temperature. It is used to determine the conditions under which a metal oxide can be reduced to its metal, helping in predicting the feasibility of reduction reactions based on whether the ?G° is negative (indicating spontaneity) at a given temperature.

Gibbs Free Energy

Gibbs free energy is a thermodynamic property that indicates the spontaneity of a reaction under constant pressure and temperature. A negative value of ?G (whether standard or non?standard) signifies that a reaction can proceed spontaneously, while a positive value suggests non-spontaneity. Understanding Gibbs free energy is crucial in evaluating which reduction processes are feasible in metallurgical operations.

Reduction Reaction

A reduction reaction is a chemical process in which a species gains electrons, often involving the removal of oxygen from a metal oxide. In metallurgical practice, reduction reactions are used to convert metal oxides into their elemental metals by using reducing agents such as carbon, carbon monoxide, or hydrogen. The effectiveness and direction of such reactions depend largely on their thermodynamic properties, particularly the Gibbs free energy change.

Standard State Conditions

Standard state conditions provide a reference point where substances are assumed to be at a set pressure (1 atm) and a specified concentration or activity (commonly chosen as 1 M for solutions). When discussing ?G° values, it is implicit that they refer to measurements under these standard conditions, which allows for consistent comparison of thermodynamic data across different reactions.

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