Consider the reaction: 2NO(g)+2H2(g)-> N2(g) + 2H2O(l) Using standard thermodynamic data at 298K, calculate the entropy change for the surrounding when 2.08 moles of NO(g) react at standard conditions. Values of S°(J/mol K) NO= 210.8 N2=191.6 H2= 130.7 H2O=69.9   S°surroundings=

Consider the reactionS(s,rhombic) + 2CO(g)SO2(g) + 2C(s,graphite)for which H° = -75.80 kJ and S° = -167.6 J/K at 298.15 K.(1) Calculate the entropy change of the UNIVERSE when 1.716 moles of S(s,rhombic) react under standard conditions at 298.15 K. Suniverse =  J/K (2) Is this reaction reactant or product favored under standard conditions?(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'.

Consider the reaction 2NH3(g) + 3N₂O(g) → 4N₂ (9) + 3H₂O(g) for which AH° = − 879.5 kJ and AS° = 288.1 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 2.344 moles of NH3(g) react under standard conditions at 298.15 K. ASuniverse = J/K 2. Is this reaction reactant or product favored under standard conditions? 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'.

Consider the reaction: Fe2O3(s) + 2Al(s) → Al2O3 (s) + 2Fe(s) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 2.00 moles of Fe₂O3(s) react at standard conditions. AS⁰ Substance AH (kJ/mol) Fe₂O3(s) -824.2 Al(s) 0.0 Al2O3(s) -1675.7 Fe(s) 0.0 surroundings J/K