3. $\mathrm{Fe}$ and $\mathrm{FeO}$ are in equilibrium with gas mixture of composition $71.8 \% \mathrm{CO}-$ $28.2 \% \mathrm{CO} 2$ at $1273 \mathrm{~K}$. Which of the two solid phases disappears if the composition of the gas is held constant and temperature of the system is increased?
$$
\begin{array}{l}
\mathrm{Fe}(\mathrm{s})+1 / 2 \mathrm{O} 2(\mathrm{~g})=\mathrm{FeO}(\mathrm{s}) \Delta \mathrm{Go}=-263700+64.35 \mathrm{~T} \mathrm{C}(\mathrm{s})+\mathrm{O} 2(\mathrm{~g})=\mathrm{CO} 2(\mathrm{~g}) \Delta \mathrm{Go}=-394100- \
0.84 \mathrm{~T} \mathrm{C}(\mathrm{s})+1 / 2 \mathrm{O} 2(\mathrm{~g})=\mathrm{CO} \Delta \mathrm{Go}=-111700-87.65 \mathrm{~T}
\end{array}
$$

Question

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Determine the direction of reaction shift**: To find out which solid phase disappears with an increase in temperature, we need to consider the sign of the temperature coefficient in the Gibbs free energy equations. ‖ ‖ 2 ⋮ **Analyze the Gibbs free energy for Fe formation**: For the reaction $\mathrm{Fe(s)} + \frac{1}{2} \mathrm{O_2(g)} = \mathrm{FeO(s)}$, the Gibbs free energy change is $\Delta G^\circ = -263700 + 64.35T$. The positive temperature coefficient (+64.35) indicates that as temperature increases, the Gibbs free energy becomes less negative, favoring the reverse reaction (decomposition of FeO). ‖ ‖ 3 ⋮ **Analyze the Gibbs free energy for CO formation**: For the reaction $\mathrm{C(s)} + \frac{1}{2} \mathrm{O_2(g)} = \mathrm{CO(g)}$, the Gibbs free energy change is $\Delta G^\circ = -111700 - 87.65T$. The negative temperature coefficient (-87.65) indicates that as temperature increases, the Gibbs free energy becomes more negative, favoring the forward reaction (formation of CO). ‖ ‖ 4 ⋮ **Compare the effects of temperature on both reactions**: Since increasing temperature favors the decomposition of FeO and the formation of CO, the equilibrium will shift to consume FeO and produce more CO and Fe. ‖ ∻Answer∻ ⚹ FeO solid phase disappears as the temperature of the system is increased. ⚹ ∻Key Concept∻ ⚹ The temperature dependence of the Gibbs free energy change determines the direction in which a reaction shifts when the temperature is changed. ⚹ ∻Explanation∻ ⚹ The positive temperature coefficient in the Gibbs free energy equation for the formation of FeO indicates that increasing temperature will favor the reverse reaction, leading to the disappearance of FeO.◊What is the relationship between the changes in Gibbs free energy and the equilibrium constant for a chemical reaction involving Fe, FeO, CO, and CO2 at 1273K?⍭ Generate me a similar question◊⚹

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