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Standard Enthalpy of Formation. * for Various Compounds. Compound. ?H?f (kJ/mol). Compound. ?H?f (kJ/mol). Compound. ?H?f (kJ/mol). Compound. ?H?f (kJ/mol). Ag2O(s). ?30.6. C2H5OH(l). ?277.6. HCl(g). ?92.3. NH4Cl(s). ?315.4. Ag2S(s). ?31.8. C2H6(g). ?84.7. HF(g). ?268.6. NH4NO3(s). ?365.1. AgBr(s). ?99.5.
20 Feb 2011 This table lists the standard enthalpies (?H°), the free energies (?G°) of formation of compounds from elements in their standard states, and the thermodynamic (third-law) entropies (S°) of compounds at 298 K. The state of the compound is specified by the following symbols: (g) - gas (l) = liquid (s) - solid
A.1. Gas-phase entropy and enthalpy values. Table A-1 lists selected entropy and enthalpy of formation values at 298 K for a number of atmospheric species. As much as possible, the values were taken from primary evaluations, that is, evaluations that develop a recommended value from the original studies. Otherwise, the
states. Substances are listed by molecular formula in a modified Hill order; all compounds not containing carbon appear first, followed by those that contain carbon. The properties tabulated are: ?fH°. Standard molar enthalpy (heat) of formation at 298.15 K in kJ/mol. ?fG°. Standard molar Gibbs energy of formation at 298.15
Standand Enthalpies of Formation & Standard Entropies of Common Compounds. Substance State. ?H? f. S?. ( kJ mol. ) ( J mol·K. ) Ag s. 0. 42.6. Ag+ aq. 105.79. 72.7. AgCl s. ?127.01. 96.2. AgBr s. ?100.4. 107.1. AgNO3 s. ?124.4. 140.9. Al s. 0. 28.3. Al+3 aq. ?538.4 ?321.7. AlCl3 s. ?704. 110.7. Al2O3 s. ?1675.7. 50.9. Ba.
Heats of Formation, or Enthalpies of Formation, are used to provide a concise collection of thermochemical data. • For consistency, enthalpy of formation data are recorded for reactions that take place under standard conditions. • Standard conditions are. – Constant books and are shown in Table 8.3 of the text (page. 221).
Standard Enthalpies of Formation. Alan D. Earhart. 11/7/2016. Substance. ?H°f (kJ/mol). Substance. ?H°f (kJ/mol). Substance. ?H°f (kJ/mol). AgCl(s). -127.0. CaSO4(s). -1434.5. N2H4(g). +95.4. Al2O3(s). -1675.7. Fe2O3(s). -824.2. N2H4(l). +50.6. CHCl3(g). -103.2. HBr(g). -36.4. N2O(g). +82.1. CH2Cl2(g). -95.5. HCl(g).
O(g): 33.58 J K?1 mol?1; H. 2. (g): 28.84. J K?1 mol?1; O. 2. (g): 29.37 J K?1 mol?1. Assume heat capacities are independent of temp T. • Answer H. 2. (g) + ?O. 2. (g) > H. 2. O(g). •. •. • Test 2.7 Estimate the standard enthalpy of formation of cyclohexene at 400 K from the data in Table 2-5. • Correct Answer: ?163 kJ mol?1
Enthalpy. H = U + PV. Enthalpy is a state function and at constant pressure: ?H = ?U + P?V and ?H = q. At constant pressure, the change in enthalpy is equal to the heat released or absorbed by the system. Exothermic: ?H < 0. Endothermic: ?H > 0. Thermoneutral: ?H = 0
31. Standard Thermodynamic Values. Formula. State of Matter. Enthalpy. (kJ/mol). Entropy (J mol/K). Gibbs Free Energy. (kJ/mol). (NH4)2O. (l). -430.70096. 267.52496. -267.10656. (NH4)2SiF6. (s hexagonal). -2681.69296. 280.24432. -2365.54992. (NH4)2SO4. (s). -1180.85032. 220.0784. -901.90304. Ag. (s). 0. 42.55128.
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