When ethene is mixed with hydrogen in the presence of a platinum catalyst, hydrogen adds across the double bond to form ethane. At room temperature, the reaction goes to completion. Predict the signs of ∆H° and ∆S° for this reaction. Explain these signs in terms of bonding and freedom of motion.

Part 1 and part 2 go together For part 2, Then use the data below to calculate ∆G rxn using free energies of formation.

A 0.582-g sample of Mg reacts with excess 1.0 M HCl (60.0 mL) according to the procedure used in this experiment. The initial and final temperatures were 24°C and 68°C. What is the ∆H of the reaction per mole of magnesium? Assume that the specific heat capacity for the solution is 4.187 J/oC∙g and that the density of the 1.0 M HCl is 1.00 g/mL. (Hints: the magnesium contributes to the mass of the solution; take care with your sig figs.) (answer: - 4.7 × 102 kJ/mol)Show your solution to this problem in the space below. It is your solution which will be graded.

Calculate the Free Gibb’s Energy, kJ/mol, at 298 K for the following reaction.  2CaSO4(s)→2CaO(s) + 2SO2(g) + O2(g) Substance ∆H(kJ/mol) ∆S (J/K mol) CaSO4(s) -1432.69 106.69 CaO(s) -635.6 39.8 SO2(g) -296.4 248.5 O2(g0 0 205.0