Calculate ΔrH⊖ and ΔrU⊖ at 298 K and ΔrH⊖ at 348 K for the hydrogenation of ethyne to ethene from the enthalpy of formation and heat capacity data. Assume the heat capacities to be constant over the temperature range, and ideal gas behavior.
The hydrogenation reaction is:
C2H2(g) + H2(g) → C2H4(g)
The thermodynamics data at 298 K are the following:
ΔfH⊖[C2H2(g)] = 226.73 kJ mol−1; Cp⊖[C2H2(g)] = 43.93 J K−1 mol−1
ΔfH⊖[C2H4(g)] = 52.26 kJ mol−1; Cp⊖[C2H4(g)] = 43.56 J K−1 mol−1
Cp⊖[H2(g)] = 28.82 J K−1 mol−1