a$)$ For above given reaction derive the empirical equation that gives the relationship between $logP{O}_2-T$ in the form of $logP=-\frac{A}{T}+B(atm)\mathrm{.}15$ pts

b$)$ For $727$ and $1127C,$ determine the equilibrium oxygen pressure values and show the $logP{O}_2-IT$ change on a diagram by indicating the phase stability regions. Using the diagram that you plotted determine the direction of reaction for $927C$ with $P{O}_2={10}^{-2}$ and $P{O}_2={10}^{-15}$atm ambient pressure values. $25$ pts

Below given reaction is in equilibrium at $1$atm total pressure.

$Fe{O}_{(s)}+C{O}_{(s)}=F{e}_{(s)}+C{O}_2(e)$

Calculate the equilibrium constants of above given reaction at $750C$ and $1250C\mathrm{.}15pts$

Calculate the heat of reaction using Van't Hoff equation from the calculated equilibrium constant value

or above given reaction, calculate the composition of gases and $($:$C{O}_2\%\}$ when the reactir brium at $1$atm total ambient pressure at $750C\mathrm{.}10pts$

a representative Ellingham diagram and show the reactions given below $($reaction #$1,$ #$2$ and by obeying the rules. $15pts$

$($#$1)F{e}_{(s)}+\frac{1}{2}{O}_{2(g)}=Fe{O}_{(s)}$

$(\frac{?}{?}$#$2)C_{(s)}+O_{2(g)}=C{O}_{2(g)}$

$(\frac{?}{?}$#$3)C_{(s)}+\frac{1}{2}{O}_{2(g)}=C{O}_{(g)}$