Using the Ksp for Ag2SO4(s) and the ΔGf° for Ag+(aq) and SO4^-2(aq), calculate the ΔGf° for...
Using the Ksp for Ag2SO4(s) and the ΔGf° for Ag+(aq) and SO4^-2(aq), calculate the ΔGf° for Ag2SO4(s). Ag2SO4(s) -> 2 Ag+(aq) + SO4^-2(aq). Ksp = 1.2 x 10-5, ΔGf° for Ag+(aq) = +77.1 kJ/mol and ΔGf° for SO4-2(aq) = 744.6 kJ/mol.
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Using the Ksp for Ag2SO4(s) and the ΔGf° for Ag+(aq) and
SO4^-2(aq), calculate the ΔGf° for...
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=
Calculate ΔG°rxn,298 and ΔGrxn,298 for the following. a) Ag+(aq) + Cl-(aq) -> AgCl (s) b) Ag+(...
Calculate ΔG°rxn,298 and ΔGrxn,298 for the following.
a) Ag+(aq) + Cl-(aq) -> AgCl (s)
b) Ag+(aq) + I-(aq) -> AgI (s)
c) Ag+(aq) + NO3-(aq) -> AgNO3 (aq)
d) Ag+(aq) + SO4 2-(aq) -> Ag2SO4(aq)
e) Ba 2+(aq) + 2Cl- (aq) + 2H2O (l) -> BaCl2 • 2H2O
f) Ba 2+(aq) + 2NO3-(aq) -> Ba(NO3)2 (aq)
ΔGo, 298 values for 1M solutions NO3 -108.74 -33.41 SO42 -744.53 -618.41 Cl -109.789 -1296.32 W2 -384.138 Anions (kJ/mol) Cations (kJ/mol) -51.57 -66.19 Ag...
a) Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its molar solubility. b) If Ksp...
a) Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its molar solubility. b) If Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its mass solubility in g solute/100g of water. Please answer a & b
The equilibrium constant for the reaction Agl(s) — Ag+ (aq) +1 (aq) is the solubility product...
The equilibrium constant for the reaction Agl(s) — Ag+ (aq) +1 (aq) is the solubility product constant, Ksp = 8.3 x 10-17 at 25°C. Calculate AG for the reaction when [Ag+]=1.5 x 10-3 M and [Br] =1.5 x 10-2 M. Is the reaction spontaneous or nonspontaneous at these concentrations? AG = 98 kJ/mol, spontaneous AG = 92 kJ/mol, nonspontaneous AG = -65 kJ/mol, spontaneous AG = 65 kJ/mol, nonspontaneous AG = -92 kJ/mol, spontaneous
Consider the equilibrium reaction: Ag2SO4(s) <=> 2Ag+ + SO4-2. Which of the following is the correct...
Consider the equilibrium reaction: Ag2SO4(s) <=> 2Ag+ + SO4-2. Which of the following is the correct equilibrium expression for this equation? [Ag+][SO4^-2}/[Ag2SO4] [Ag+]^2 [SO4^-2}/[Ag2SO4] (wrong answer) [Ag+][SO4^-2} [Ag+]^2 [SO4^-2}
ksp for Ag2SO4=1.6*10^-5 WhatſAg*) is needed to just begin precipitating Ag2SO4(s) from a .053 M SO42-...
ksp
for Ag2SO4=1.6*10^-5
WhatſAg*) is needed to just begin precipitating Ag2SO4(s) from a .053 M SO42- (aq) solution? O 8.7 x 10M O 9.2 x 10-4M O 1.7 x 102M O 3.0 x 10-4M O 1.5 x 10-4M 3 pts Question 9 What is the charge of Fe in the complex [Fe(CN)2(SO4)25?? 0 +6 O +1 +3 +2 o -3
Given that Ksp for AgI(s) = 8.3 × 10−17 and Kf for [Ag(CN)2]− = 1.0 ×...
Given that Ksp for AgI(s) = 8.3 × 10−17 and Kf for [Ag(CN)2]− = 1.0 × 1021 at 25°C, what is the ΔG° for the following reaction at the same temperature? AgI(s) + 2 CN−(aq) ⇌ [Ag(CN)2]−(aq) + I−(aq) A. –300 kJ/mol B. –248 kJ/mol C. –152 kJ/mol D. –28 kJ/mol E. +13 kJ/mol
Consider the following Gibbs energies at 25 "C Substance Ag (aq) Cr(aq) AgCI(s) Br(aq) AgBr(s) 77.1...
Consider the following Gibbs energies at 25 "C Substance Ag (aq) Cr(aq) AgCI(s) Br(aq) AgBr(s) 77.1 - 131.2 - 109.8 - 104.0 -96.9 (a) Calculate AG rn for the dissolution of AgCl(s). (b) Calculate the solubility-product constant of AgCl Number Number kJ mol (c) Calculate Δ3rxn for the dissolution of AgBr(s). (d) Calculate the solubility-product constant of AgBr Number Number kJ mol
I just need help with question D, finding the ksp value. AgCI (s) = Ag+ (aq)...
I just need help with question
D, finding the ksp value.
AgCI (s) = Ag+ (aq) + Cl^- (aq) lg the data in the table given: Calculate the DeltaHdegree (in kJ/mol) for dissolving AgCI in aqueous solution. Calculate the ASdegree (in J/molK) for dissolving AgCI in aqueous solution. Calculate the AGdegree (in kJ/mol) for dissolving AgCI in aqueous solution at 25degreeC. What is the value for Ksp at this temperature?
Given the following reactions, AgBr(s) = Ag+ (aq) + Br(aq) Ksp = 5.8 x 10-13 Ag+...
Given the following reactions, AgBr(s) = Ag+ (aq) + Br(aq) Ksp = 5.8 x 10-13 Ag+ (aq) + 2 CN"(aq) = Ag(CN)2(aq) Kf = 9.5 x 1021 determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN"(aq) =Ag(CN)2(aq) + Br(aq) Answer: 1.2E21 Check
Calculate ΔG°rxn,298 and ΔGrxn,298 for the following.
a) Ag+(aq) + Cl-(aq) -> AgCl (s)
b) Ag+(aq) + I-(aq) -> AgI (s)
c) Ag+(aq) + NO3-(aq) -> AgNO3 (aq)
d) Ag+(aq) + SO4 2-(aq) -> Ag2SO4(aq)
e) Ba 2+(aq) + 2Cl- (aq) + 2H2O (l) -> BaCl2 • 2H2O
f) Ba 2+(aq) + 2NO3-(aq) -> Ba(NO3)2 (aq)
ΔGo, 298 values for 1M solutions NO3 -108.74 -33.41 SO42 -744.53 -618.41 Cl -109.789 -1296.32 W2 -384.138 Anions (kJ/mol) Cations (kJ/mol) -51.57 -66.19 Ag...
The equilibrium constant for the reaction Agl(s) — Ag+ (aq) +1 (aq) is the solubility product constant, Ksp = 8.3 x 10-17 at 25°C. Calculate AG for the reaction when [Ag+]=1.5 x 10-3 M and [Br] =1.5 x 10-2 M. Is the reaction spontaneous or nonspontaneous at these concentrations? AG = 98 kJ/mol, spontaneous AG = 92 kJ/mol, nonspontaneous AG = -65 kJ/mol, spontaneous AG = 65 kJ/mol, nonspontaneous AG = -92 kJ/mol, spontaneous
ksp
for Ag2SO4=1.6*10^-5
WhatſAg*) is needed to just begin precipitating Ag2SO4(s) from a .053 M SO42- (aq) solution? O 8.7 x 10M O 9.2 x 10-4M O 1.7 x 102M O 3.0 x 10-4M O 1.5 x 10-4M 3 pts Question 9 What is the charge of Fe in the complex [Fe(CN)2(SO4)25?? 0 +6 O +1 +3 +2 o -3
Consider the following Gibbs energies at 25 "C Substance Ag (aq) Cr(aq) AgCI(s) Br(aq) AgBr(s) 77.1 - 131.2 - 109.8 - 104.0 -96.9 (a) Calculate AG rn for the dissolution of AgCl(s). (b) Calculate the solubility-product constant of AgCl Number Number kJ mol (c) Calculate Δ3rxn for the dissolution of AgBr(s). (d) Calculate the solubility-product constant of AgBr Number Number kJ mol
I just need help with question
D, finding the ksp value.
AgCI (s) = Ag+ (aq) + Cl^- (aq) lg the data in the table given: Calculate the DeltaHdegree (in kJ/mol) for dissolving AgCI in aqueous solution. Calculate the ASdegree (in J/molK) for dissolving AgCI in aqueous solution. Calculate the AGdegree (in kJ/mol) for dissolving AgCI in aqueous solution at 25degreeC. What is the value for Ksp at this temperature?
Given the following reactions, AgBr(s) = Ag+ (aq) + Br(aq) Ksp = 5.8 x 10-13 Ag+ (aq) + 2 CN"(aq) = Ag(CN)2(aq) Kf = 9.5 x 1021 determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN"(aq) =Ag(CN)2(aq) + Br(aq) Answer: 1.2E21 Check
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