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.
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) −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+(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 = 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 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 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- (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 × 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 - 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