Calculate the standard free energies of formation of Cl- in aqueous solution and of AgCl (s).
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![The balanced equation and expression for Ksp AgCl (s) Agt (a) Cl (aq) Ksp Ag]C] Please note that you have all the free energy](http://img.homeworklib.com/questions/a93fa870-7026-11ea-b281-97c5b3aa646b.png?x-oss-process=image/resize,w_560)
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Calculate the standard free energies of formation of Cl- in aqueous
solution and of AgCl (s).
Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq)...
Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq) Using the standard free energy of formation values (ΔG⁰f) from the appendix, calculate the Kc value for this reaction. Calculate the ΔG for the dissolving of AgCl in water at 25⁰C when: [Ag+]=[Cl-]= 1.00 x 10-4M
Calculate Ksp for Ag2S(s), then using standard free energies of formation, calculate molar solubility of Ag+...
Calculate Ksp for Ag2S(s), then using standard free energies of formation, calculate molar solubility of Ag+ and S2-. Delta G of Ag2S = -40.7KJ/mol Delta G of Ag+ = 77.11KJ/mol Delta G of S2- = 83.7KJ/mol
AgCl dissolves in aqueous solutions of S2O3 2- via formation of complex, Ag(S2O3) 3- AgCl(s) +...
AgCl dissolves in aqueous solutions of S2O3 2- via formation of complex, Ag(S2O3) 3- AgCl(s) + 2 S2O3 2- (aq) → Ag(S2O3)2 3- (aq) + Cl-(aq). Using Ksp and Kf, Calculate the value of KC for the above reaction. Kf for Ag(S2O3)2 3- is 2.9 x 1013 ; Ksp for AgCl is 1.8 x 10-10. Show the sequence of equations that yield the above reaction. Please help :)
Calculate ΔG° for the following reactions at 25°C using the standard free energies of formation of...
Calculate ΔG° for the following reactions at 25°C using the standard free energies of formation of the reactants and products. CS2(l) → CS2(g)
Consider the Gibbs energies at 25 ∘C. SubstanceSubstance ΔG∘f (kJ⋅mol−1)ΔGf∘ (kJ·mol−1) Ag+(aq)Ag+(aq) 77.177.1 Cl−(aq)Cl−(aq) −131.2−131.2 AgCl(s)AgCl(s)...
Consider the Gibbs energies at 25 ∘C. SubstanceSubstance ΔG∘f (kJ⋅mol−1)ΔGf∘ (kJ·mol−1) Ag+(aq)Ag+(aq) 77.177.1 Cl−(aq)Cl−(aq) −131.2−131.2 AgCl(s)AgCl(s) −109.8−109.8 Br−(aq)Br−(aq) −104.0−104.0 AgBr(s)AgBr(s) −96.9−96.9 (a) Calculate ΔG∘rxn for the dissolution of AgCl(s)AgCl(s). kJ⋅mol−1 (b) Calculate the solubility-product constant of AgCl. K= (c) Calculate ΔG∘rxnΔGrxn∘ for the dissolution of AgBr(s)AgBr(s). kJ⋅mol−1kJ⋅mol−1 (d) Calculate the solubility-product constant of AgBr. K=K=
63) Use standard free energies of formation to calculate ΔG° at 25°C for each reaction in Problem...
answer #63 by using #61
63) Use standard free energies of formation to calculate ΔG° at 25°C for each reaction in Problem 61. How do the values of AG° calcu- lated this way compare to those calculated from ΔΗ' and AS? Which of the two methods could be used to determine how ΔG changes with temperature? İN or each reaction, calculate Δ Hon, Δ-mn, and ΔGon at 25°C and state whether the reaction is spontaneous. If the reaction is not...
) Use standard Gibbs energies of formation to calculate the standard reaction Gibbs energies at 298...
) Use standard Gibbs energies of formation to calculate the standard reaction Gibbs energies at 298 K of the reactions (i) Zn(s)+Cu2+ (aq) → Zn2+ (aq)+Cu(s) (ii) C12H2201(s)+1202(8)-12CO2(g)+11H2O0)
Starting with the standard free energies of formation from the following table, calculate the values of...
Starting with the standard free energies of formation from the
following table, calculate the values of ΔG° and E°cell of the
following reactions.
Substance
ΔΔG°f
(kJ/mol)
FeO(s)
-255.2
H2(g)
0
Fe(s)
0
H2O(l)
-237.2
Pb(s)
0
O2(g)
0
H2SO4(aq)
-744.5
PbSO4(s)
-813.0
1) FeO(s) +H2(g) ----Fe(s) +H2O(l)
change in G=18kj
E Cell= v
2) 2Pb(s)+O2(g)+2H2SO4(aq)--------2PbSO4(s)+2H2O(l)
change in G=-611.4
E°cell
= V
Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following...
Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following reactions. How do the values of ΔG∘ calculated this way compare to those calculated from ΔH∘ and ΔS∘? Which of the two methods could be used to determine how ΔG∘ changes with temperature? Essay answers are limited to about 500 words (3800 characters maximum, including spaces).
Consider the following hypothetical reaction at 310 K. Standard free energies of formation are given in...
Consider the following hypothetical reaction at 310 K. Standard free energies of formation are given in parentheses. B C G° = –46.0 kJ/mol (?) (176.4 kJ/mol) Calculate the standard free energy of formation of compound B. a) 222.4 kJ/mol b) –222.4 kJ/mol c) 130.4 kJ/mol d) –130.4 kJ/mol e) none of these Please show work
answer #63 by using #61
63) Use standard free energies of formation to calculate ΔG° at 25°C for each reaction in Problem 61. How do the values of AG° calcu- lated this way compare to those calculated from ΔΗ' and AS? Which of the two methods could be used to determine how ΔG changes with temperature? İN or each reaction, calculate Δ Hon, Δ-mn, and ΔGon at 25°C and state whether the reaction is spontaneous. If the reaction is not...
) Use standard Gibbs energies of formation to calculate the standard reaction Gibbs energies at 298 K of the reactions (i) Zn(s)+Cu2+ (aq) → Zn2+ (aq)+Cu(s) (ii) C12H2201(s)+1202(8)-12CO2(g)+11H2O0)
Starting with the standard free energies of formation from the
following table, calculate the values of ΔG° and E°cell of the
following reactions.
Substance
ΔΔG°f
(kJ/mol)
FeO(s)
-255.2
H2(g)
0
Fe(s)
0
H2O(l)
-237.2
Pb(s)
0
O2(g)
0
H2SO4(aq)
-744.5
PbSO4(s)
-813.0
1) FeO(s) +H2(g) ----Fe(s) +H2O(l)
change in G=18kj
E Cell= v
2) 2Pb(s)+O2(g)+2H2SO4(aq)--------2PbSO4(s)+2H2O(l)
change in G=-611.4
E°cell
= V
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