Calculate ΔHrº and ΔUrº at 298K and ΔHrº at 348 K for the hydrogenation (adding hydrogen to unsaturated molecules) of ethyne (acetylene) to ethane (ethylene). Assume that heat capacities to be constant over the temperature range involved. ΔHrº(H2(g)) = -285.83 kJ mol⁻¹, ΔCp,rº(H2(g)) = 28.82 kJ K⁻¹ mol⁻¹ ΔHrº(C2H2(g)) = -1300 kJ mol⁻¹, ΔCp,rº(C2H2(g)) = 43.93 kJ K⁻¹ mol⁻¹ ΔHrº(C2H4(g)) = -1411 kJ mol⁻¹, ΔCp,rº(C2H4(g)) = 43.56 kJ K⁻¹ mol⁻¹ a) Start by writing out the hydrogenation overall reaction, and each of the balanced combustion reactions. b) Show the ΔHrº and ΔUrº of the abovementioned hydrogenation reaction at 298K. Show all steps. c) Show ΔHrº at 348 K.