Use values from Table 1 (page ) to calculate standard values of AH run and AGran for both NH.CH and CaCl2. ΔΗ" κη: AG How do your calculated Hex and AG values using experimental data compare to the standard values? Using your results for trial 1, calculate the temperature (in Kelvin) CaCl2 becomes spontaneous. Is the dissolution of CaCl2 spontaneous above or below the temperature calculated above? Was this process spontaneous at room temperature? Conclusion: In the space below, summarize your average calculated values for AH, A5, and AG for each salt. Describe what the sign of each value tells you about the dissolution of that salt.
Ammonium Chloride, NHACI Triali Calcium Chloride, CaCl2 Trial Trial II Trial 11 Mass salt (8) 2.0108 g 2.0763g 2.07844 Moles salt Mass water (8) Mass solution (8) 27.07639 27.0784 g Initial Temp (°C) Final Temp (°C) AT (C) 2.0764g 10.08760 mol 0.03881 mor 0.01873 mol 0.01871 mol 25g 259 25g 25g 27.01089 27.01695 25.00°C 95.00°C 15.00°C 25.00°C 21.12€ 21.01°C 39.34°C 39.37°C -3.88°C -3.90°C 14.34°C 14.37 'e |438.495 452.0165 -1624.6655 -1627.4443 11661.968 kJ / mot 11646.895 kJ/mod-86741.324 kJ/mol -87009.300 kJ/mol AS = 75.3 I molk Adran = -46.8 J/molk 1-10,789.695 W/mod-10803.8 kJ/mol -73209.104 kJ/mol -73055.88 kJ/mol -10726.7475 KJ/mol -72182.492 KJ/mol Arun (1) AH(kJ/mol) nan ASørn (J/mol K) calculated from table 1 AGA (kJ/mol) yan Average AGran(kJ/mol)
Table 1: NH.Cl(s) NH. + (aq) Cl - (aq) CaCl2 (s) Ca2+ (aq) Thermodynamic data from textbook AHO: (kJ/mol) -314.4 -132.5 - 167.2 -795.8 -542.9 Sº (J/mol K) 94.6 113.4 56.5 104.6 -55.2 AG: (kJ/mol) -202.8 -79.3 - 131.2 -748.1 -553.0
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