Consider the following information at 25 ºC: AgBr(s) + e- → Ag(s) + Br-(aq) Eº(AgBr(s),Ag(s)) = 0.07133 V Ag+(aq) + e- → Ag(s) Eº(Ag+(aq),Ag(s)) = 0.7996 V What is the value of the solubility product equilibrium constant Ksp(AgBr) of silver bromide? AgBr(s) ↔ Ag+(aq) + Br-(aq) Ksp(AgBr)
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Consider the following information at 25 ºC: AgBr(s) + e- → Ag(s) + Br-(aq) Eº(AgBr(s),Ag(s)) =...
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
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
Given the following reactions, AgBr(s) Ag (aq) + Br(aq) Ag*(aq)2 CN (aq)=Ag(CN)2(aq) K 1.2E+21 determine the equilibrium constant for the reaction below AgBr(s)2 CN-(aq)= Ag(CN)2 (aq) Brr(aq) Ksp 5.4E-13
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=
Question 5 Calculate Eº cell for the reaction below, 2 AgBr(aq) + 2 Hg(1) 2 Ag(s) + Hg2Br2(5) given the following standard reduction potentials. Hg2Br2(s) + 2 - 2 Hg(1) + 2 Br"(aq) E = +0.140 V AgBr(aq) + e - Ag(s) + Br" (aq) E = +0.071 V O a. -0.211 V O b. +0.069 V O C. +1.97 v O d. -0.069 V O e. +0.211 V Question 6 Given the following substances and their vapor pressures at...
all 5&6 5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
For the following redox reaction at 25 ºC, Eº cell = 2.24 V. Calculate the equilibrium constant, K. Mg(s) + Pb 2+ (aq) → Mg 2+ (aq) + Pb(s)
Consider the Gibbs energies at 25 'C AGi (kJ mol) Substance Ag (aq) 77.1 CI (aq) -131.2 AgCls) -109.8 Br (aq) -104.0 -96.9 AgBr(s) (a) Calculate AGn for the dissolution of AgC1(s) kJ mol (b) Calculate the solubility-product constant of AgCl. K = (c) Calculate AGxn for the dissolution of AgBr(s). kJ mol (d) Calculate the solubility-product constant of AgBr. K =
Question 22 (5 points) Given the following half reactions: - AgBr(s) + e- Ag+ (aq) + e- Ag(s) + Br- (aq) E° = 0.07V → Ag (s) E° = 0.80V - Calculate the Ksp for PbSO4 at 25 degrees C. Please enter your answer in scientific notation, such as 1.2E10 or 1.2E-10 and keep two significant figures.
Item 10: Question (10 pts.) Given the following reactions, AgBr(s) = Ag+(aq) + Br-(aq) Kap = 5.4E-13 Ag+ (aq) + 2 CN-(aq) — Kp = 1.2E+21 Ag(CN), (aq) determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN- (aq) = Ag(CN)2 (aq) + Br(aq) Submit Submit and Next O: Mark this question for later review. - Skip to Previous