Calculate the enthalpy of vaporization of water at its normal boiling point. Δ S ° [H 2O( )] = 69.9 J/K ⋅mol and Δ S ° [H 2O(g)] = 188.8 J/K ⋅mol.

■ The disorder in a solid is greater than that in a liquid. ( ✓ or X ) ■ The tendency of a process to occur naturally is called equilibrium. (✓ or X ) ▪ A spontaneous change happens unidirectional or in one way. For a reverse change to occur, work always has to be done. (✓ or X) ■ For a spontaneous change to occur, time is not a factor. A spontaneous reaction can be a rapid or very slow reaction. (✓or X ) ■ If the system is not in the equilibrium, a spontaneous change is unavoidable. The change will continue until the system reaches the state of equilibrium. (✓or X ) ■ Thermal heat transfers between cold and hot reservoirs in both directions. (✓ or X ) ■ Absolute zero kelvin is attainable. (✓or X)

Calculate the temperature, in Kelvins, at which the decomposition of calcium carbonate becomes spontaneous (you do not need to include temperature units in your answer): CaCO3 (s) --> CaO (s) + CO2 (g) ΔHo = 179.0 kJ ΔSo = 160.2 J/K

Calculate for the ΔS given the values of  ΔHo = +119.2 kJ,  ΔGo= +13.4 kJ at 298.5 K of temperature. CO(NH2)2(aq) + H2O(l) ----> CO2(g) + 2 NH3(g)

Calculate ΔGrxn at 375 K for the reaction below when PCO = 2.20 atm and PCO2 = 5.10 atm.  Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)        ΔG°rxn = –28.0 kJ

50.0 ml of 0.600 M K2SO4 solution is added to 100.0 ml of 0.400 M Ba(NO3)2 solution. The temperature of the solutions increases from 21.00oC to 22.26oC. Calculate ΔH for the reaction below. Assume the density of all solutions as 1.00 g/ml K2SO4 (aq) + Ba(NO3)2 (aq) → BaSO4 (s) + 2 KNO3 (aq)

Calcium ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) Ca (s) 0 0 41.4 Ca (g) 178.2 144.3 158.9 Ca2+ (g) 1925.9     CaC2 (s) -59.8 -64.9 70.0 CaCO3 (s, calcite) -1206.9 -1128.8 92.9 CaCl2 (s) -795.8 -748.1 104.6 CaF2 (s) -1219.6 -1167.3 68.9 CaH2 (s) -186.2 -147.2 42.0 CaO (s) -635.1 -604.0 39.8 CaS (s) -482.4 -477.4 56.5 Ca(OH)2 (s) -986.1 -898.5 83.4 Ca(OH)2 (aq) -1002.8 -868.1 -74.5 Ca3(PO4)2 (s) -4126.0 -3890.0 241.0 CaSO4 (s) -1434.1 -1321.8 106.7 CaSiO3 (s) -1630.0 -1550.0 84.0       Carbon ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) C (s, graphite) 0 0 5.7 C (s, diamond) 1.9 2.9 2.4 C (g) 716.7 671.3 158.1 CCl4 (l) -135.4 -65.2 216.4 CCl4 (g) -102.9 -60.6 309.9 CHCl3 (l) -134.5 -73.7 201.7 CHCl3 (g) -103.1 -70.3 295.7 CH4 (g) -74.8 -50.7 186.3 CH3OH (g)…

For a particular reaction, Δ?=−14.20 kJ and Δ?=−198.5 J/K. Calculate Δ? for this reaction at 298 K