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A process at constant T and P can be described as spontaneous if AG <0 and...
A process at constant T and P can be described as spontaneous if ΔG < 0...
A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.) PCl3(g) + Cl2(g) → PCl5(g) ΔHf° (kJ mol-1) -287.0 -374.9...
A process at constant T and P can be described as spontaneous if ΔG < 0...
A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.) 3 PbO2(s) → Pb3O4(s) + O2(g) ΔHf° (kJ mol-1) -277.0...
Gibbs free energy change AG is defined as AG= AH-TAS. For a spontaneous process, AG<0. For...
Gibbs free energy change AG is defined as AG= AH-TAS. For a spontaneous process, AG<0. For a. reversible reaction at equilibrium, AG = 0. The equilibrium constant K of the reversible reaction is relate- AG"=-RTIn(K). Symbol 40" refers to thermodynamics standard condition: 298 K and 1 atm. Exercise:consider the following reaction: bo:pfoiex 2 HNO:(aq)+NO(g)- 3 NO2(g) + H2O(I) AH=+136.5 kJ; AS = +287.5 J/K a. Below what temperature does the following reaction becomes nonspontaneous? niliod sis anotsole s ob io...
(9) A spontaneous process has the change of free energy (a) AG>0 (c) AG = 0...
(9) A spontaneous process has the change of free energy (a) AG>0 (c) AG = 0 (b) AG <O (d) AH>0 and AS <O (10) A chemical reaction has AH = 10 kJ. AS = 50 J/K at temperature T = 300 K. the reaction AG = J. (a) 5000 (b) -5000 (c) 10000 (d) 50 (11) For reaction: Ag (s) + 2 Cl2 (g) Ag° (aq) +CI (aq), the standard free energy of formation: AGf° (Ag*) = 77.1 kJ/mol,...
(9) A spontaneous process has the change of free energy (a) AG > 0 (b) AG <0 (c) AG = 0 (d) AH >0 and AS &...
(9) A spontaneous process has the change of free energy (a) AG > 0 (b) AG <0 (c) AG = 0 (d) AH >0 and AS <0 (10) A chemical reaction has AH = 10 kJ, AS = 50 J/K at temperature T = 300 K, the reaction AG = (a) 5000 (b)-5000 (c) 10000 (d) 50 (11) For reaction : Ag (s) + 1/2 Cl2 (g) = Agt (aq) + CI+ (aq), the standard free energy of formation: AGE"...
Chapter 18 Thermodynamics Homework 1.Predict the sign of AS for each process: a) The boiling of water b)2HgO(s)-2Hg(I) + 02(s) c) CaCO, (s)CaO(s)+ CO (g) 2. Is the following process spontaneous o...
Chapter 18 Thermodynamics Homework 1.Predict the sign of AS for each process: a) The boiling of water b)2HgO(s)-2Hg(I) + 02(s) c) CaCO, (s)CaO(s)+ CO (g) 2. Is the following process spontaneous or nonspontaneous at a given temperature? NaNO,(s) ->NaNO,(aq) 3. If a reaction has ΔS < 0 and ΔΗ < 0 will the reaction always be spontaneous, spontaneous at low T, spontaneous at high T, or never spontaneous? 4.Consider this reaction: Calculate ΔG at 25 °C and determine whether the...
8. Vaporization is a reversible process at constant T&P. AG=0. The heat of vaporization of water...
8. Vaporization is a reversible process at constant T&P. AG=0. The heat of vaporization of water at the boiling point is 40,900 kJ/mol. Calculate S, with the proper label, of vaporizat 1. Calculate S, with the proper label, of vaporization at the same temperature and I atm. 0=40,900 2TAS 40,900. 00 >40,900-27305 40,900,000 /molek -273- 273 151 109)/molk - As= 149816.8J/molok. 273 = 149816.85/mo1*
10. Given the following table: Compound NO: (g) N:O (g) AHP (J mol) AGP (J mol) 51.84 33.85 9.66 98.29 For t...
10. Given the following table: Compound NO: (g) N:O (g) AHP (J mol) AGP (J mol) 51.84 33.85 9.66 98.29 For the reaction: N:Oa (g) eo 2NO: (g) (a) Use the information in the Table to calculate AG for the reaction (b) Use the information in the Table to calculate AH" for the reaction (c) Calculate K, at 25 C. (d) Calculate K, at 1600 °C. (Assume AH to be temperature independent) (e) Calculate the degree of dissociation, a, of...
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction:...
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction: NO2(g) + CO(g) NO(g) + CO2(g) 0 -222 kJ 0-990 kJ 0 - 199 kJ O-1211 kJ O-420 kJ AG; (kJ/mol ) at 25°c AH; Sº (kJ/mol) (KJ/K mol) AG, (kJ/mol) at 25°c ΔΗ: sº (kJ/mol) (kJ/kmol) 0.0 -20.6 H2S (g) -33.6 +0.2057 -814.0 H2SO4(0) +0.1569 -690.1 0.0 Hg(e) 0.0 +0.0760 -90.8 Hgo (3) -58.6 +0.0703 12 () 0.0 0.0 +0.1161 0.0 K(s) +0.0642...
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction:...
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction: NO2(g) + CO(g) + NO(g) + CO2(g) O-420 kJ 0-222 kJ O-1211 kJ 0-199 kJ 0-990 kJ 3 pts Question 27 What is the pH of .731 M H2CO3 (aq)? 8.4 O 5.2 O 3.3 O 6.5 10.7 Table 6 - Thermodynamic Data of 12.0 M HOH ZOH is added to Ag(s) AgBr(s) Agcl(s) AgI (8) AgNO, () Ag20(8) Al(a) Al,0, () Ba (3)...
Gibbs free energy change AG is defined as AG= AH-TAS. For a spontaneous process, AG<0. For a. reversible reaction at equilibrium, AG = 0. The equilibrium constant K of the reversible reaction is relate- AG"=-RTIn(K). Symbol 40" refers to thermodynamics standard condition: 298 K and 1 atm. Exercise:consider the following reaction: bo:pfoiex 2 HNO:(aq)+NO(g)- 3 NO2(g) + H2O(I) AH=+136.5 kJ; AS = +287.5 J/K a. Below what temperature does the following reaction becomes nonspontaneous? niliod sis anotsole s ob io...
(9) A spontaneous process has the change of free energy (a) AG>0 (c) AG = 0 (b) AG <O (d) AH>0 and AS <O (10) A chemical reaction has AH = 10 kJ. AS = 50 J/K at temperature T = 300 K. the reaction AG = J. (a) 5000 (b) -5000 (c) 10000 (d) 50 (11) For reaction: Ag (s) + 2 Cl2 (g) Ag° (aq) +CI (aq), the standard free energy of formation: AGf° (Ag*) = 77.1 kJ/mol,...
(9) A spontaneous process has the change of free energy (a) AG > 0 (b) AG <0 (c) AG = 0 (d) AH >0 and AS <0 (10) A chemical reaction has AH = 10 kJ, AS = 50 J/K at temperature T = 300 K, the reaction AG = (a) 5000 (b)-5000 (c) 10000 (d) 50 (11) For reaction : Ag (s) + 1/2 Cl2 (g) = Agt (aq) + CI+ (aq), the standard free energy of formation: AGE"...
Chapter 18 Thermodynamics Homework 1.Predict the sign of AS for each process: a) The boiling of water b)2HgO(s)-2Hg(I) + 02(s) c) CaCO, (s)CaO(s)+ CO (g) 2. Is the following process spontaneous or nonspontaneous at a given temperature? NaNO,(s) ->NaNO,(aq) 3. If a reaction has ΔS < 0 and ΔΗ < 0 will the reaction always be spontaneous, spontaneous at low T, spontaneous at high T, or never spontaneous? 4.Consider this reaction: Calculate ΔG at 25 °C and determine whether the...
8. Vaporization is a reversible process at constant T&P. AG=0. The heat of vaporization of water at the boiling point is 40,900 kJ/mol. Calculate S, with the proper label, of vaporizat 1. Calculate S, with the proper label, of vaporization at the same temperature and I atm. 0=40,900 2TAS 40,900. 00 >40,900-27305 40,900,000 /molek -273- 273 151 109)/molk - As= 149816.8J/molok. 273 = 149816.85/mo1*
10. Given the following table: Compound NO: (g) N:O (g) AHP (J mol) AGP (J mol) 51.84 33.85 9.66 98.29 For the reaction: N:Oa (g) eo 2NO: (g) (a) Use the information in the Table to calculate AG for the reaction (b) Use the information in the Table to calculate AH" for the reaction (c) Calculate K, at 25 C. (d) Calculate K, at 1600 °C. (Assume AH to be temperature independent) (e) Calculate the degree of dissociation, a, of...
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction: NO2(g) + CO(g) NO(g) + CO2(g) 0 -222 kJ 0-990 kJ 0 - 199 kJ O-1211 kJ O-420 kJ AG; (kJ/mol ) at 25°c AH; Sº (kJ/mol) (KJ/K mol) AG, (kJ/mol) at 25°c ΔΗ: sº (kJ/mol) (kJ/kmol) 0.0 -20.6 H2S (g) -33.6 +0.2057 -814.0 H2SO4(0) +0.1569 -690.1 0.0 Hg(e) 0.0 +0.0760 -90.8 Hgo (3) -58.6 +0.0703 12 () 0.0 0.0 +0.1161 0.0 K(s) +0.0642...
Use Table 6 values to calculate AGº (in kJ) at 2000 K for the following reaction: NO2(g) + CO(g) + NO(g) + CO2(g) O-420 kJ 0-222 kJ O-1211 kJ 0-199 kJ 0-990 kJ 3 pts Question 27 What is the pH of .731 M H2CO3 (aq)? 8.4 O 5.2 O 3.3 O 6.5 10.7 Table 6 - Thermodynamic Data of 12.0 M HOH ZOH is added to Ag(s) AgBr(s) Agcl(s) AgI (8) AgNO, () Ag20(8) Al(a) Al,0, () Ba (3)...
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