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

Under 1 atm total pressure of $\mathrm{CO}_{2}+\mathrm{CO}$ answer the given questions:
a) For the reaction (i), calculate the "heat of reaction"( by using Van't Hoff equation) and equilibrium constants $(K p)$ at given temperatures $(415,625$, $835,1045$ and $1255 \mathrm{~K})$.
b) Using the Bouduard reaction (ii), for each temperature, calculate the equilibrium gas composition. Plot temperature versus $\% \mathrm{CO}$.
c) For the reaction (i), calculate equilibrium gas composition for each temperature. Plot temperature versus $\% \mathrm{CO}$.
d) Using / overlapping the plotted graphs, explain the reduction behavior of $\mathrm{FeO}$ with $\mathrm{CO}$.
$$
\begin{array}{l}
\mathrm{Fe}+1 / 2 \mathrm{O}_{2}=\mathrm{FeO} \
\mathrm{C}+\mathrm{O}_{2}=\mathrm{CO}_{2} \
\mathrm{C}+1 / 2 \mathrm{O}_{2}=\mathrm{CO}
\end{array}
$$
$$
\begin{array}{l}
\Delta G^{\circ} \mathrm{T}=-263700+64,35 \mathrm{~T} \
\Delta \mathrm{G}^{\circ} \mathrm{T}=-394100-0,84 \mathrm{~T} \
\Delta \mathrm{G}^{\circ} \mathrm{T}=-111700-87,65 \mathrm{~T}
\end{array}
$$

Question

$$
\begin{array}{l}
\mathrm{FeO}+\mathrm{CO}=\mathrm{Fe}+\mathrm{CO}_{2} \
\mathrm{CO}_{2}+\mathrm{C}=2 \mathrm{CO}
\end{array}
$$

Under 1 atm total pressure of $\mathrm{CO}_{2}+\mathrm{CO}$ answer the given questions:
a) For the reaction (i), calculate the "heat of reaction"( by using Van't Hoff equation) and equilibrium constants $(K p)$ at given temperatures $(415,625$, $835,1045$ and $1255 \mathrm{~K})$.
b) Using the Bouduard reaction (ii), for each temperature, calculate the equilibrium gas composition. Plot temperature versus $\% \mathrm{CO}$.
c) For the reaction (i), calculate equilibrium gas composition for each temperature. Plot temperature versus $\% \mathrm{CO}$.
d) Using / overlapping the plotted graphs, explain the reduction behavior of $\mathrm{FeO}$ with $\mathrm{CO}$.
$$
\begin{array}{l}
\mathrm{Fe}+1 / 2 \mathrm{O}_{2}=\mathrm{FeO} \
\mathrm{C}+\mathrm{O}_{2}=\mathrm{CO}_{2} \
\mathrm{C}+1 / 2 \mathrm{O}_{2}=\mathrm{CO}
\end{array}
$$
$$
\begin{array}{l}
\Delta G^{\circ} \mathrm{T}=-263700+64,35 \mathrm{~T} \
\Delta \mathrm{G}^{\circ} \mathrm{T}=-394100-0,84 \mathrm{~T} \
\Delta \mathrm{G}^{\circ} \mathrm{T}=-111700-87,65 \mathrm{~T}
\end{array}
$$

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Calculate the standard Gibbs free energy change for reaction (i)**: Use the given $\Delta G^\circ T$ values for the formation of $\mathrm{FeO}$, $\mathrm{CO_2}$, and $\mathrm{CO}$ to find the $\Delta G^\circ$ for the reaction $\mathrm{FeO} + \mathrm{CO} = \mathrm{Fe} + \mathrm{CO_2}$. ‖ ‖ 2 ⋮ **Use Van't Hoff equation**: The Van't Hoff equation relates the equilibrium constant $K_p$ to the standard Gibbs free energy change $\Delta G^\circ$ by $\Delta G^\circ = -RT \ln K_p$, where $R$ is the gas constant and $T$ is the temperature in Kelvin. ‖ ‖ 3 ⋮ **Calculate $K_p$ for each temperature**: Rearrange the Van't Hoff equation to solve for $K_p$ at each given temperature. ‖ ‖ 4 ⋮ **Calculate the heat of reaction**: The heat of reaction at constant pressure, or enthalpy change $\Delta H$, can be estimated from the temperature dependence of $K_p$ using the Van't Hoff isochore, which relates $\ln K_p$ to $1/T$. ‖ ∻Answer∻ ⚹ The equilibrium constants $K_p$ and the heat of reaction for each temperature will be calculated based on the Van't Hoff equation and the Gibbs free energy changes. ⚹ ∻Key Concept∻ ⚹ Van't Hoff equation and Gibbs free energy ⚹ ∻Explanation∻ ⚹ The Van't Hoff equation relates the equilibrium constant of a reaction to the temperature and the standard Gibbs free energy change. ⚹ ∻Solution∻ ‖ 1 ⋮ **Use the Boudouard reaction (ii)**: Write the expression for the equilibrium constant $K_p$ for the Boudouard reaction $\mathrm{CO_2} + \mathrm{C} = 2 \mathrm{CO}$. ‖ ‖ 2 ⋮ **Calculate $K_p$ for each temperature**: Use the standard Gibbs free energy change for the Boudouard reaction to calculate $K_p$ at each given temperature. ‖ ‖ 3 ⋮ **Determine the equilibrium gas composition**: Use the calculated $K_p$ values to find the equilibrium composition of $\mathrm{CO}$ and $\mathrm{CO_2}$ at each temperature. ‖ ‖ 4 ⋮ **Plot temperature versus $\% \mathrm{CO}$**: Create a graph with temperature on the x-axis and the percentage of $\mathrm{CO}$ in the equilibrium gas mixture on the y-axis. ‖ ∻Answer∻ ⚹ The equilibrium gas composition for the Boudouard reaction and the corresponding plot of temperature versus $\% \mathrm{CO}$ will be provided. ⚹ ∻Key Concept∻ ⚹ Equilibrium constant and gas composition ⚹ ∻Explanation∻ ⚹ The equilibrium constant of a reaction determines the composition of the products and reactants at equilibrium. ⚹ ∻Solution∻ ‖ 1 ⋮ **Use reaction (i)**: Write the expression for the equilibrium constant $K_p$ for the reaction $\mathrm{FeO} + \mathrm{CO} = \mathrm{Fe} + \mathrm{CO_2}$. ‖ ‖ 2 ⋮ **Calculate the equilibrium gas composition**: Use the previously calculated $K_p$ values to find the equilibrium composition of $\mathrm{CO}$ and $\mathrm{CO_2}$ for reaction (i) at each temperature. ‖ ‖ 3 ⋮ **Plot temperature versus $\% \mathrm{CO}$**: Create a graph with temperature on the x-axis and the percentage of $\mathrm{CO}$ in the equilibrium gas mixture for reaction (i) on the y-axis. ‖ ∻Answer∻ ⚹ The equilibrium gas composition for reaction (i) and the corresponding plot of temperature versus $\% \mathrm{CO}$ will be provided. ⚹ ∻Key Concept∻ ⚹ Equilibrium constant and gas composition for reaction (i) ⚹ ∻Explanation∻ ⚹ The equilibrium constant of reaction (i) determines the composition of $\mathrm{CO}$ and $\mathrm{CO_2}$ at equilibrium. ⚹ ∻Solution∻ ‖ 1 ⋮ **Analyze the plotted graphs**: Compare the plots of temperature versus $\% \mathrm{CO}$ for both the Boudouard reaction and reaction (i). ‖ ‖ 2 ⋮ **Explain the reduction behavior**: Discuss how the equilibrium compositions of $\mathrm{CO}$ and $\mathrm{CO_2}$ influence the reduction of $\mathrm{FeO}$ by $\mathrm{CO}$ at different temperatures. ‖ ∻Answer∻ ⚹ The reduction behavior of $\mathrm{FeO}$ with $\mathrm{CO}$ will be explained by analyzing the plotted graphs of temperature versus $\% \mathrm{CO}$ for both reactions. ⚹ ∻Key Concept∻ ⚹ Influence of equilibrium compositions on reduction behavior ⚹ ∻Explanation∻ ⚹ The equilibrium compositions of $\mathrm{CO}$ and $\mathrm{CO_2}$ determine the efficiency of the reduction of $\mathrm{FeO}$ by $\mathrm{CO}$ at different temperatures. ⚹◊What is the significance of the Van't Hoff equation in calculating the heat of reaction and equilibrium constants in chemical reactions?⍭ Generate me a similar question◊

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