At 298 K, the following chemical reaction:
$$
\mathrm{CO} (\mathbf{g}) + \mathrm{H}_{2}\mathrm{O} (\mathbf{g}) = \mathrm{CO}_{2} (\mathbf{g}) + \mathrm{H}_{2} (\mathbf{g})
$$
has the following thermodynamic properties:
$$
\Delta_{t} H_{m}^{\Theta}(298 \, \mathrm{K}) = -41.162 \, \mathrm{kJ} \cdot \mathrm{mol}^{-1}, \quad \Delta_{t} G_{m}^{\Theta}(298 \, \mathrm{K}) = -28.522 \, \mathrm{kJ} \cdot \mathrm{mol}^{-1}.
$$
The molar heat capacities at constant pressure, $C_{p, m}^{\Theta}(T)$, for each gaseous substance are as follows:
$$
C_{p, m}^{\Theta}(\mathrm{CO_{2}}) = \left[ 26.648 + 42.26 \times 10^{-3} (\frac{T}{K}) - 14.247 \times 10^{-6} (\frac{T}{K})^{2} \right] \, \mathrm{J} \cdot \mathrm{K^{-1}} \cdot \mathrm{mol^{-1}}
$$
$$
C_{p, m}^{\Theta}(\mathrm{H_{2}}) = \left[ 29.08 + 0.84 \times 10^{-3} (\frac{T}{K}) + 2.013 \times 10^{-6} (\frac{T}{K})^{2} \right] \, \mathrm{J} \cdot \mathrm{K^{-1}} \cdot \mathrm{mol^{-1}}
$$
$$
C_{p, m}^{\Theta}(\mathrm{CO}) = \left[ 27.61 + 5.02 \times 10^{-3} (\frac{T}{K}) \right] \, \mathrm{J} \cdot \mathrm{K^{-1}} \cdot \mathrm{mol^{-1}}
$$
$$
C_{p, m}^{\Theta}(\mathrm{H_{2}O}) = \left[ 30.13 + 11.30 \times 10^{-3} (\frac{T}{K}) \right] \, \mathrm{J} \cdot \mathrm{K^{-1}} \cdot \mathrm{mol^{-1}}
$$
Please calculate the values of $\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}(1273 \, \mathrm{K})$ and $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}(1273 \, \mathrm{K})$. Is it beneficial to increase the temperature for the positive reaction?

Options:
A. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 2 2 0 5 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=7 5 3 4 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ decreases, which is unfavorable for the forward reaction.
B. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-2 9 8 1 3 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=7 6 3 9 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ increases, which is favorable for the forward reaction.
C. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 2 2 0 5 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=6 2 8 9 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ decreases, which is unfavorable for the forward reaction.
D. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 4 8 0 5 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=6 8 8 3 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ increases, which is favorable for the forward reaction.
E. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 0 5 4 0 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=8 7 2 3 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ increases, which is favorable for the forward reaction.
F. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 4 0 0 7 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=7 0 1 2 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ decreases, which is favorable for the forward reaction.
G. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 2 2 0 5 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta} ( 1 2 7 3 \, \mathrm{K} )=6 8 8 3 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ increases, which is unfavorable for the forward reaction.
H. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 2 2 0 5 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=7 1 2 0 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ decreases, which is favorable for the forward reaction.
I. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 5 1 0 0 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=6 0 0 0 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ decreases, which is unfavorable for the forward reaction.
J. $$
\begin{array} {l} {{{\Delta_{\mathrm{r}} H_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=-3 2 2 0 5 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ {{{\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}( 1 2 7 3 \, \mathrm{K} )=7 5 0 2 \, \mathrm{J} \cdot\mathrm{m o l}^{-1}}}} \\ \end{array}
$$
As the temperature increases, the value of $\Delta_{\mathrm{r}} G_{\mathrm{m}}^{\Theta}$ decreases, which is favorable for the forward reaction.
Answer: G