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
Given that Ksp for AgI(s) = 8.3 × 10−17 and Kf for [Ag(CN)2]− = 1.0 ×...
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
What is the molar solubility of AgI in 0.750 M NH3? Ksp for AgI is 8.3∙10-17, and Kf for Ag(NH3)2+ is 1.70∙107
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
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
A solution contains 2.2×10−4 M Ag+ and 1.7×10−3 M Pb2+. If NaI is added, will AgI(Ksp=8.3×10−17) or PbI2(Ksp=7.9×10−9) precipitate first? AgI. My question is: Specify the concentration of I− needed to begin precipitation.
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.
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021 for [Ag(CN)2], calculate the equilibrium constant for the reaction: Agl(s) + 2 CN (aq)[Ag(CN2] (aq) + I'(aq) c) Calculate the molar solubility of Agl in a 0.100 M NaCN solution. (20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021...
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) 4.9 x 10'M b)24x10 M c)5.8x 1010 M )1.2 x 10 M 19. Which one of the following compounds will have the lowest molar solubility in pur water? b) CuS, Ksp 1.27x103 d) ZnS, Ksp = 1.6 x 10-24 a) PbS, Ksp 9.04 x 102 e) Al(OH)s, Ksp 3 x 1034 What is the molar solubility, i.e. [Fe , in a saturated aqueous solution of 20. Fe(OH)20) Fe(OH(s)Fe2+(aa) + 201H (ag), Ksp 4.87 x 101" a) 2.44 x 1017...
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