Example: Estimate Keg at 400°C for • AS-198.3 J/K Ο ΔΗ° = -92.38 ΚJ • AG-33.32 kJ rxn eq N₂+ 3H2 → 2NH3 • Keg at 298 K = 6.9 × 105 eq

Consider the reaction 2NaOH(aq) + H₂(g)—2Na(s) + 2H₂O(1) for which AH° = 368.6 kJ and AS° = 15.30 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.290 moles of NaOH(aq) react under standard conditions at 298.15 K. ASuniverse = (2) Is this reaction reactant or product favored under standard conditions? J/K (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'.

Use the values you measured for Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH°1: -452kJ, and MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) ΔH°2: -133kJ, with the known ΔH°3 = ΔH°f(H2O, l) = –286 kJ/mol, to find your experimental ΔH°f(MgO), as: [f MgO] Mg(s) + ½O2(g) → MgO(s) ΔH°f(MgO) = ΔH°1 – ΔH°2 + ΔH°3 = ______ kJ/mol

Using values from Appendix C of your textbook, calculate the value of Keq at 298 K for each of the following reactions: (a) 6 C(graphite) + 6 H₂O(1) C6H1206(5) Keq=1.1E- (b) 2 NO(g) + Cl₂(g) = 2 NOCI(g) Kea (c) 2 N₂Ha(g) + 2 H₂O(1) = 4 NHy(9) + O₂(g) Kea