$$
\begin{array}{l}
\mathrm{FeO}+\mathrm{CQ}=\mathrm{Fe}+\mathrm{CO} 2 \
\mathrm{CO} 2+\mathrm{C}=2 \mathrm{CO}
\end{array}
$$

Answer the following questions by taking the total CO2+CO gas pressure in the system by 1 atm.
Answer the questions given for a total pressure of $1 \mathrm{~atm} \mathrm{CO} 2+\mathrm{CO}$.
Explain the reduction behavior of FeO with CO by using/superimposing the plotted graphs.
$$
\begin{array}{l}
\mathrm{Fe}+12 \mathrm{O} 2=\mathrm{FeO}, \Delta \mathrm{G}^{\circ} \mathrm{T}=-263700+64,35 \mathrm{~T} \
\mathrm{C}+\mathrm{O} 2=\mathrm{CO} 2, \Delta \mathrm{G}^{\circ} \mathrm{T}=-394100-0,84 \mathrm{~T} \
\mathrm{C}+12 \mathrm{O} 2=\mathrm{CO}, \Delta \mathrm{G}^{\circ} \mathrm{T}=-111700-87,65 \mathrm{~T}
\end{array}
$$

Question

$$
\begin{array}{l}
\mathrm{FeO}+\mathrm{CQ}=\mathrm{Fe}+\mathrm{CO} 2 \
\mathrm{CO} 2+\mathrm{C}=2 \mathrm{CO}
\end{array}
$$

Answer the following questions by taking the total CO2+CO gas pressure in the system by 1 atm.
Answer the questions given for a total pressure of $1 \mathrm{~atm} \mathrm{CO} 2+\mathrm{CO}$.
Explain the reduction behavior of FeO with CO by using/superimposing the plotted graphs.
$$
\begin{array}{l}
\mathrm{Fe}+12 \mathrm{O} 2=\mathrm{FeO}, \Delta \mathrm{G}^{\circ} \mathrm{T}=-263700+64,35 \mathrm{~T} \
\mathrm{C}+\mathrm{O} 2=\mathrm{CO} 2, \Delta \mathrm{G}^{\circ} \mathrm{T}=-394100-0,84 \mathrm{~T} \
\mathrm{C}+12 \mathrm{O} 2=\mathrm{CO}, \Delta \mathrm{G}^{\circ} \mathrm{T}=-111700-87,65 \mathrm{~T}
\end{array}
$$

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Identify the reactions involved**: The reduction of FeO with CO is described by the first chemical equation, and the equilibrium between CO2 and CO is described by the second equation. ‖ ‖ 2 ⋮ **Understand the role of Gibbs free energy**: The change in Gibbs free energy ($\Delta G^\circ$) for a reaction indicates the spontaneity of the reaction at standard conditions. Negative $\Delta G^\circ$ values suggest that the reaction is spontaneous. ‖ ‖ 3 ⋮ **Calculate the Gibbs free energy for each reaction at a given temperature**: Use the provided equations for $\Delta G^\circ T$ to calculate the Gibbs free energy for each reaction at a specific temperature. ‖ ‖ 4 ⋮ **Plot the Gibbs free energy vs. temperature**: By plotting $\Delta G^\circ T$ against temperature for each reaction, we can determine the temperature at which the reduction of FeO with CO becomes spontaneous. ‖ ‖ 5 ⋮ **Explain the reduction behavior using the graphs**: Superimpose the graphs to find the intersection points, which indicate the temperatures at which the reactions are in equilibrium. The reduction of FeO with CO will be spontaneous below the temperature at which the $\Delta G^\circ T$ for the reaction becomes negative. ‖ ∻Answer∻ ⚹ Without the actual graphs, we cannot provide a specific temperature at which the reduction of FeO with CO is spontaneous. However, the process involves calculating the Gibbs free energy for each reaction at various temperatures, plotting these values, and analyzing the graphs to determine the temperature range where the reduction is favorable. ⚹ ∻Key Concept∻ ⚹ Gibbs free energy and spontaneity of reactions ⚹ ∻Explanation∻ ⚹ The Gibbs free energy change for a reaction helps predict the spontaneity of the reaction. When $\Delta G^\circ$ is negative, the reaction is spontaneous under standard conditions. By plotting $\Delta G^\circ T$ against temperature, we can determine the conditions under which a reaction will occur spontaneously. ⚹◊Can you calculate the equilibrium constant $K_{eq}$ for the reaction FeO + CO = Fe + CO$_2$ at a temperature $T$?⍭ Generate me a similar question◊

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