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The equilibrium constant for the reaction Agl(s) — Ag+ (aq) +1 (aq) is the solubility product...
(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...
The equilibrium constant for the equation Ag+ (aq) + 2NH, (aq) =[Ag(NH),]+(aq) is Kf = 2.5 x 103 M-2 at 25.0 °C. Calculate the value of AGixn at 25.0 °C. C AG = k Is the reaction spontaneous under standard conditions? kJ/mol J/mol no O yes Calculate the value of AGrxn at 25.0 °C when [Ag+] = 0.00138 M, (NH2) = 0.438 M, and [[Ag(NH3)2]+] = 0.00739 M. Is the reaction spontaneous under these conditions? AGrxn = kJ/mol O yes...
Find the solubility of Agl in 2.5 M NH3 (Ksp of Agl = 8.3 x 10-17; Kf of Ag(NH3)2+ = 1.7 x 107 Enter your answer in scientific notation. 1x 10 m
9. What is the molar solubility of Agl in 0.500 M NH3? Ksp for Agl is 8.3-10-17, and Kf for Ag(NH3)2is 1.70.107
a and b please 2. The equilibrium constant for the dissociation of Ag,CO, (s) + 2 Ag+ + CO; ? is K.-8.1 x 10-12 at 25°C. a) Calculate AG for the reaction when (Agt) = 1.0 x 102 M and [CO, ) = 1.0 X 10M. (4pts) Ans: Ans: b) (1pt) Is the reaction spontaneous or nonspontaneous at these concentrations?
Be sure to answer all parts. Calculate the molar solubility and the solubility in g/L of Agl at 25°C. The Ksp of Agl is 8.3 x 10-17. x 10 M Enter your answer in scientific notation. x 10 g/L Enter your answer in scientific notation.
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)
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=
* 1) Use the solubility product constant, Ksp, of magnesium carbonate at 25°C to calculate AGo for the reaction MgCO,(s) Mg2 (aq)+CO, 2(aq), KsD 6.8x10-6 Is this process reactant- or product-favored? #2) If in the system above, [Mg2+] 0.0015 M and CO1 0.0012 M, what is AG at 25oC? Is the reaction spontaneous or non-spontaneous? Explain your answer!
1. (3pts.) Complete and balance the nuclear equation in+U - Br+3n+ 2. The equilibrium constant for the dissociation of As.CO, (s) + 2 Ag+CO, isk=8.1 10-at 25°C. a) Calculate AG for the reaction when Agtl -1.0 x 102 M and CO, 9-10 x 10 M. (4pts) Ans: b) (pt) is the reaction spontaneous or onspontaneous at these concentrations? Ans: 3. (4pts) Nitrosyl chloride (NOCI) decomposes at elevated temperatures according to the equation below; INOCHE 2NO(g) + Calculate K, for this...