Copper melts at 1083°C. Droplets of liquid Cu had been supercooled to 847°C before isothermal solidification occurred. 1. Calculate the enthalpy change of the system associated with the isothermal solidification of 1 mole of supercooled copper at 847°C. 2. Calculate entropy change of the system associated with the isothermal solidification of 1 mole of supercooled copper at 847°C. 3. Calculate the entropy change of the surroundings associated with the isothermal solidification of 1 mole of supercooled copper at 847°C. 4. Calculate the total entropy change (system and surrounding) for isothermal solidification of supercooled copper at 847°C. Comment on the results. At 1083°C, AHL-s = -12,958- L→S Cp (Liquid Cu) = 31.35 mole J mole.K Cp (Solid Cu) = 22.61 + 6.27 × 10-³T ) J mole.K

A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of  144.0°C  and constant total pressure. Then, he measures the reaction enthalpy  ΔH  and reaction entropy  ΔS  of the first reaction, and the reaction enthalpy  ΔH  and reaction free energy  ΔG  of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate  ΔG  for the first reaction and  ΔS  for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. →+C3H8g5O2g+3CO2g4H2Ol =ΔH−2220.kJ =ΔS−5322.JK =ΔGkJ Which is spontaneous?   this reaction     the…

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'.

Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids Cations Cl--131.228 I--51.57 NO3--108.74 SO4-2-744.53 Ag+77.107 AgCl -109.789 -66.19 -33.41 -618.41 Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt).Observations (Rxn or No Rxn). S or support and R for Refute Cations Cl- I- NO3- SO4-2 Ag+         Ba+2