Interpretation:
The substances having zero value for the free energy of formation
Concept introduction:
Free energy is the term that is used to explain the total energy content in a
Where,
Standard free energy of formation is the change in free energy for the formation of one mole of substance in its standard state. The standard state is
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Chemistry: Atoms First
- 17. For which of the following highly exothermic processes would you expect AH" and AG* to be about the same? (a) 2 Al(s) + 3/2 02(g) - Al;0:(s) (c) 2 Na(s) + 2 H20(1) → 2 N2OH(aq) + H2(g) (d) 2 NO(g) - N;O(g) (e) 2 Al(s) + Fe2O;(s) - 2 Fe(s) + Al;Oa(s) (b) 2 Ha(g) + Ozl8) - 2 H;0(g)arrow_forwardCalculate AS values for the following reactions by using tabulated Sº values from Appendix C. (a) 2 PCly(g) + O₂(g) = 2 POCI (9) AS133.0 X 3/K (b) C₂H4(9) + H₂(g) = C₂H6(9) AS = -120.8✔ 1/K (c) CaCO3(s)=Ca0(s) + CO₂(g) AS 160.2✔ J/K (d) Be(OH)₂(s)= Be0(s) + H₂O(g) AS 157.1 X J/Karrow_forward(ii) Given the following information, (a) Given the data below (for 298 K) calculate the free energy of formation 4G° of H,0, in the gas phase at that temperature. (b) Calculate the value of Keg for the reaction at 298 K. AH° (kJ mol') AS° (J K' mol') H2O(g) -241.8 188.8 H2(g) 130.6 O2(g) 205.1 o oarrow_forward
- The diagram shows G as a function of Q at 25°C for: GE 6. m H2O(1) = H20(g) 29. What is AG at point 4? (A) AG> AGo 5. (B) AG = AG° 4 3 (C)) AG < AG° 1arrow_forwardThe Haber process for the production of ammonia involves the equilibriumN2(g) + 3 H2(g)⇌ 2 NH3(g)For this reaction, ΔH° = -92.38 kJ and ΔS° = -198.3 J/K. Assume that ΔH° and ΔS° for this reaction do not change withtemperature. (a) Predict the direction in which ΔG for the reaction changes with increasing temperature. (b) Calculate ΔG at25 °C and at 500 °C.arrow_forward20.15 Without using Appendix B, predict the sign of ASº for (a) Ag+(aq) + CI^(aq) (b) KBr(s) – AgCI(s) KBr(aq) CH2 H,C-CH2(g) (c) CH3CH=CH2(g)arrow_forward
- Calculate AS values for the following reactions by using tabulated Sº values from Appendix C.. (a) C₂H4(9) + H₂(g) = C₂H6(9) Asº = J/K (b) 2 CH₂OH(g) + 3 0₂(g) = 2 CO₂(g) + 4H₂O(g) AS⁰ = 3/K (c) 2 PC13(g) + O₂(g) =2 POCI3(9) AS⁰ = J/K (d) N₂04(0) = 2 NO₂(9) AS⁰ = J/Karrow_forward3. (a) Use the data given below and calculate AHO, ASO, A Gº, and Kp at 25° C for the reaction: CO (g) + 3 H₂ (g) - → CH4 (g) + H₂O (g) (b) Calculate AG for the reaction at 250 °C. (c) At what temperature (°C) is AG equal to zero? In what temperature range is this reaction product- favored? Compound CO (g) H₂(g) CH4 (g) H₂O (g) AH°, kJ/mol -110.52 0 -74.81 -241.82 So, J/mol K 197.67 130.68 186.264 188.83arrow_forwardCalculate the value of K, for the reaction 2N₂(g) + O₂(g) 2N₂O(g) at 298.15 K and 1573 K. Thermodynamic data for N₂O(g) are: AH, = 82.05 kJ/mol; S = 219.9 J/mol K; AG, = 104.2 kJ/mol. (a) 298.15 K (b) 1573 K Number 10 Numberarrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax