In this problem you will analyze the dry$-$reforming reaction to produce hydrogen:

$C{O}_{2(g)}+C{H}_{4(g)}$harr$2H_{2(g)}+2C{O}_{(g)}$

Thermodynamic information of relevant species at $T_R=25C$ and at $\frac{1}{b}ar$ is below.

Assume this is an ideal gas system, and that the $C{p}_i$ is a function of temperature according to the

following equation:

$\frac{C_{Pj}^g}{R}\{T\}=A_i+B_{i}T+C_i{T}^2+\frac{D_i}{T^2}$

The $A_4,B_1,C_i,$ and $D_i$ constants for each species are listed below:

D$.$ Consider a closed system with one mole of each reactant $(N_{0.CH,0}=1(mol),N_{0.CO2\mathrm{.}0}=1(mol)).$

What would be the total Gibbs free energy of this ideal gas system at a pressure of $1$ bar

and at a temperature of $298K?($Work on the space provided on next page.$)$

What would be the total Gibbs free energy of the system if the conversion of $C{H}_4$ is $0\mathrm{.}45?$

E$.$ In industry, this reaction is commonly carried out at temperatures atzo $950K.$

Calculate $H_{rxn,}{S}_{\text{r}\text{a}\text{n}}$ and $G_{\text{r}\text{a}\text{n}}$ at $950K$ and $\frac{1}{b}ar.$

$H_{rxn}\{950K\}=,S_{\text{r}\text{a}\text{n}}\{950K\}=$

$G_{rxn}\{950K\}=,$