Given the following enthalpy change values for the reactions...

Given the following enthalpy change values for the reactions below: A + B → 2C ; ΔrH = 170.5 kJ mol^-1 E + F → C + 2D ; ΔrH = -268.5 kJ mol^-1 1/2 E + G → H ; ΔrH = 496.6 kJ mol^-1 Calculate ΔrH for the following reaction (in kJ mol^-1) using Hess's Law: A + B + 4G + 4D → 4H + 2F

The enthalpy changes of the following reactions can be measured: $$\begin{aligned} \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+3 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{g}) &+2 \mathrm{H}_{2} \mathrm{O}(\ell) \\ \Delta_{r} H^{\circ} &=-1411.1 \mathrm{kJ} / \mathrm{mol}-\mathrm{r} \mathrm{xn} \\ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\ell)+3 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\ell) \\ \Delta_{r} H^{\circ}=-1367.5 \mathrm{kJ} / \mathrm{mol}-\mathrm{rxn} \end{aligned}$$ (a) Use these values and Hess's law to determine the enthalpy change for the reaction $$\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\ell)$$ (b) Draw an energy level diagram that shows the relationship between the energy quantities involved in this problem.