![Formula SU/(K-mol 160 TABLE 16.1 Standard Molar Entropies for Some Common Substances at 25 °C Substance Formula Sº 1/(K.mol)]](http://img.homeworklib.com/questions/23783400-fc54-11ea-b952-51ee52886ca5.png?x-oss-process=image/resize,w_560)
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please answer 17a,b,c
17. Using values for the standard enthalpies of formation (AHY) and standard molar...
17. Using values for the standard enthalpies of formation (AH:9) and standard molar entropy (439) on...
17. Using values for the standard enthalpies of formation (AH:9) and standard molar entropy (439) on the Appendix, calculate the following thermodynamic values for the complete combustion of ethanol: (10 points) C2H5OH(g) + 302(g) → 2CO2(g) + 3H2O(g) a) The standard enthalpy change (AHº) b) The standard entropy change (AS) c) Use values from a) and b) above to calculate AGO at 298K d) Is this reaction spontaneous at 298K under standard conditions?
Can Be Used to calculate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A,...
Can Be Used to calculate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A, G, for various hstances at 298.15 K and one har 1057 Substance Formula 4,6°/kJ-mol- acetylene ammonia C.H,() NH,(g) CHCI) Br(e) CH) C(s) C(s) CO (8) CO(g) 209.20 - 16.367 124.35 3.126 -17.15 2.900 benzene bromine butane carbon(diamond) carbon(graphite) carbon dioxide carbon monoxide ethane ethanol ethene glucose hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide hydrogen peroxide iodine methane methanol CH(E) сHOH(1) CH (8) CH...
eNaICUrate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A,G", for various substances at...
eNaICUrate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A,G", for various substances at 298.15 K and one bar. 1057 Substance Formula 4,G"/kJ-mol acetylene сН.0 NH,(g) ammonia 209.20 benzene -16.367 с,н.Ф 124.35 bromine Br (g) 3.126 butane C,Hog) -17.15 carbon(diamond) C(s) 2.900 carbon(graphite) C(s) carbon dioxide cO(g) -394.389 carbon monoxide COg) -137.163 ethane СН, С Н, ОнФ сН. Ф C,H,0,(s) HBr(g) НСK -32.82 ethanol -174.78 ethene 68.421 glucose -910.52 hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide -53.513...
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous...
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
1) Calculate AH (250°C) for the formation of ammonia gas from nitrogen gas and hydrogen gas...
1) Calculate AH (250°C) for the formation of ammonia gas from nitrogen gas and hydrogen gas Substance Enthalpy value (kJ/mole) Entropy value K-mole) 1925 1306 191.5 Ammonia gas Hydrogen gas Nitrogen gas (write rxn with phase labels) 1) Calculate the standard Enthalpy change at 25.0°C Gaseous water (-241.8 kJ/mole) plus Carbon graphitel( 0.0 kJ/mole) yields hydrogen gas (0.0kJ/mole) plus carbon dioxide gas(-393.5 kJ/mole) Calcium carbonate (marble chips) reacts with hydrochloric acid to produce carbon dioxide gas, water and calcium chloride....
Using enthalpies of formation (Appendix C), calculate ΔH ° for the following reaction at 25°C. Also...
Using enthalpies of formation
(Appendix C), calculate ΔH ° for the following reaction at 25°C.
Also calculate ΔS ° for this reaction from standard entropies at
25°C. Use these values to calculate ΔG ° for the reaction at this
temperature. COCl2(g) + H2O(l ) h CO2(g) + 2HCl(g).
Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kW/mol) 0 AG: (kJ/mol) 0 S° (J/mol-K) 20.87 ΔΗ, (kJ/mol) -946.3 - 33422 AG; {kj/mol) --859,3 -2793 (J/mol-K)...
I hope the answer is clear and correct thanks Question 1 (1 point) What is the...
I hope the answer is clear and correct thanks
Question 1 (1 point) What is the change in enthalpy (in kJ mol'?) for the following reaction F2(g) + Cabr,(s) CaF() + Brz(1) O 1) -112 kJmo12 O2) 504 kJmo11 03) -504 kJmol 1 04) 537 kJmo11 O 5) -537 kJmol'i Question 2 (1 point) What is true about the following reaction at 25°C? F,(g) + 2HCl(g) 2 2017(g) + H (9) Ahrº=76 kJ mol'i Asr°=-10.13 J mol'i Ki Agrº=79 kJ...
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C....
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C. See Appendix C for data. Fe(s) + Cu2+ (aq) = Fe2+ (aq) + Cu(s) Find equilibrium constan + K at 25°C Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kJ/mol) AG; (kJ/mol (J/mol-K) 20.87 Substance or lon Ba(OH),(s) ΔΗ: (kJ/mol) -946.3 --3342.2 AG (kJ/mol) -859.3 -2793 (J/mol K) 107.1 427 Ba(OH), 8H,O(s) BaSO (8) - 1473.2 -1362.3 132.2...
#6-9 6. Calculate the enthalpy change for the reaction given below, using thermodynamic tables in your...
#6-9
6. Calculate the enthalpy change for the reaction given below, using thermodynamic tables in your book (Appendix 2): CH(g)+02(B) HO(g) + CO,(g) (not balanced) 7. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide: CaCO3 CO2+ CaO Using data from the textbook (Apendix 2), determine the heat of reaction. 8. When potassium chloride reacts with oxygen under the right conditions, potassium chlorate is formed: 2 KCI+3 02 2KCIO3 Using data from the textbook (Appendix 2),...
17. Using values for the standard enthalpies of formation (AH:9) and standard molar entropy (439) on the Appendix, calculate the following thermodynamic values for the complete combustion of ethanol: (10 points) C2H5OH(g) + 302(g) → 2CO2(g) + 3H2O(g) a) The standard enthalpy change (AHº) b) The standard entropy change (AS) c) Use values from a) and b) above to calculate AGO at 298K d) Is this reaction spontaneous at 298K under standard conditions?
Can Be Used to calculate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A, G, for various hstances at 298.15 K and one har 1057 Substance Formula 4,6°/kJ-mol- acetylene ammonia C.H,() NH,(g) CHCI) Br(e) CH) C(s) C(s) CO (8) CO(g) 209.20 - 16.367 124.35 3.126 -17.15 2.900 benzene bromine butane carbon(diamond) carbon(graphite) carbon dioxide carbon monoxide ethane ethanol ethene glucose hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide hydrogen peroxide iodine methane methanol CH(E) сHOH(1) CH (8) CH...
eNaICUrate Equilibrium Constants TABLE 26.1 Standard molar Gibbs energies of formation, A,G", for various substances at 298.15 K and one bar. 1057 Substance Formula 4,G"/kJ-mol acetylene сН.0 NH,(g) ammonia 209.20 benzene -16.367 с,н.Ф 124.35 bromine Br (g) 3.126 butane C,Hog) -17.15 carbon(diamond) C(s) 2.900 carbon(graphite) C(s) carbon dioxide cO(g) -394.389 carbon monoxide COg) -137.163 ethane СН, С Н, ОнФ сН. Ф C,H,0,(s) HBr(g) НСK -32.82 ethanol -174.78 ethene 68.421 glucose -910.52 hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide -53.513...
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
1) Calculate AH (250°C) for the formation of ammonia gas from nitrogen gas and hydrogen gas Substance Enthalpy value (kJ/mole) Entropy value K-mole) 1925 1306 191.5 Ammonia gas Hydrogen gas Nitrogen gas (write rxn with phase labels) 1) Calculate the standard Enthalpy change at 25.0°C Gaseous water (-241.8 kJ/mole) plus Carbon graphitel( 0.0 kJ/mole) yields hydrogen gas (0.0kJ/mole) plus carbon dioxide gas(-393.5 kJ/mole) Calcium carbonate (marble chips) reacts with hydrochloric acid to produce carbon dioxide gas, water and calcium chloride....
Using enthalpies of formation
(Appendix C), calculate ΔH ° for the following reaction at 25°C.
Also calculate ΔS ° for this reaction from standard entropies at
25°C. Use these values to calculate ΔG ° for the reaction at this
temperature. COCl2(g) + H2O(l ) h CO2(g) + 2HCl(g).
Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kW/mol) 0 AG: (kJ/mol) 0 S° (J/mol-K) 20.87 ΔΗ, (kJ/mol) -946.3 - 33422 AG; {kj/mol) --859,3 -2793 (J/mol-K)...
I hope the answer is clear and correct thanks
Question 1 (1 point) What is the change in enthalpy (in kJ mol'?) for the following reaction F2(g) + Cabr,(s) CaF() + Brz(1) O 1) -112 kJmo12 O2) 504 kJmo11 03) -504 kJmol 1 04) 537 kJmo11 O 5) -537 kJmol'i Question 2 (1 point) What is true about the following reaction at 25°C? F,(g) + 2HCl(g) 2 2017(g) + H (9) Ahrº=76 kJ mol'i Asr°=-10.13 J mol'i Ki Agrº=79 kJ...
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C. See Appendix C for data. Fe(s) + Cu2+ (aq) = Fe2+ (aq) + Cu(s) Find equilibrium constan + K at 25°C Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kJ/mol) AG; (kJ/mol (J/mol-K) 20.87 Substance or lon Ba(OH),(s) ΔΗ: (kJ/mol) -946.3 --3342.2 AG (kJ/mol) -859.3 -2793 (J/mol K) 107.1 427 Ba(OH), 8H,O(s) BaSO (8) - 1473.2 -1362.3 132.2...
#6-9
6. Calculate the enthalpy change for the reaction given below, using thermodynamic tables in your book (Appendix 2): CH(g)+02(B) HO(g) + CO,(g) (not balanced) 7. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide: CaCO3 CO2+ CaO Using data from the textbook (Apendix 2), determine the heat of reaction. 8. When potassium chloride reacts with oxygen under the right conditions, potassium chlorate is formed: 2 KCI+3 02 2KCIO3 Using data from the textbook (Appendix 2),...
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