Calculate the standard reaction enthalpy for the following reaction.
$\begin{array}{ll}\mathrm{CH}_{4}(\mathrm{~g}) +\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{CO}(\mathrm{g}) +3 \mathrm{H}_{2}(\mathrm{~g}) \\\text { Given: }2 \mathrm{H}_{2}(\mathrm{~g}) +\mathrm{CO}(\mathrm{g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{l}) & \Delta H^{\circ}=-128.3 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} \\2 \mathrm{CH}_{4}(\mathrm{~g}) +\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{CH}_{3} \mathrm{OH}(\mathrm{l}) & \Delta H^{\circ}=-328.1 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} \\2 \mathrm{H}_{2}(\mathrm{~g}) +\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) & \Delta H^{\circ}=-483.6 \mathrm{~kJ} \cdot \mathrm{mol}^{-1}\end{array}$

Question

Calculate the standard reaction enthalpy for the following reaction.

\begin{array}{ll}\mathrm{CH}_{4}(\mathrm{~g}) +\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{CO}(\mathrm{g}) +3 \mathrm{H}_{2}(\mathrm{~g}) \\\text { Given: }2 \mathrm{H}_{2}(\mathrm{~g}) +\mathrm{CO}(\mathrm{g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{l}) & \Delta H^{\circ}=-128.3 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} \\2 \mathrm{CH}_{4}(\mathrm{~g}) +\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{CH}_{3} \mathrm{OH}(\mathrm{l}) & \Delta H^{\circ}=-328.1 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} \\2 \mathrm{H}_{2}(\mathrm{~g}) +\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) & \Delta H^{\circ}=-483.6 \mathrm{~kJ} \cdot \mathrm{mol}^{-1}\end{array}

Quizplus · Accepted Answer

The Answer of Calculate the standard reaction enthalpy for the following reaction. $\begin{array}{ll}\mathrm{CH}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g})\ \text { Given: }2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}(\mathrm{g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{l}) & \Delta H^{\circ}=-128.3 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} \ 2 \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{CH}_{3} \mathrm{OH}(\mathrm{l}) & \Delta H^{\circ}=-328.1 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} \ 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) & \Delta H^{\circ}=-483.6 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} \end{array}$ A) +155.5 kJ.mol^-¹ B) + 216 kJ.mol^-¹ C) +412.1 kJ.mol^-¹ D) +42.0 kJ.mol^-¹ E) +206.1 kJ.mol^-¹

Calculate the Standard Reaction Enthalpy for the Following Reaction A) +1555 KJ