the first Kc is higher .because the concentration of the prduct is more ,the value of Kc is also higher
therfore in the first case the concentration of [Ag^+] is more at equilibrium.
Consider these reactions: AgCl(s) Ag^+ (aq) + Cl^- (aq K_c = 1.8 Times 10^-10 Ag_2 CrO_4...
7. (5 pts) The equilibrium constant for dissociation of silver chloride AgCl (s) + Ag (aq) + Cl(aq) Is 1.8x10. Find concentration of silver and chloride ions in saturated aqueous solution of silver chloride.
AgCl (s) + --> <-- Ag + (aq) + Cl- (aq) Shown above is information about the dissolution of AgCl in water at 298 K. In a chemistry lab a student wants to determine the value of s, the molar solubility of AgCl, by measuring [Ag+] in a saturated solution prepared by mixing excess AgCl and distilled water. How would the results of the experiment be altered if the student mixed excess AgCl with tap water (in which [Cl-] =...
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ Calculate ΔH for formation of 0.490 mol of AgCl by this reaction. Calculate ΔH for the formation of 7.50 g of AgCl. Calculate ΔH when 9.23×10−4 mol of AgCl dissolves in water.
Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag+(aq)+Cl−(aq)→AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solution to completely precipitate the silver?
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ A.) Calculate ΔH for formation of 0.100 mol of AgCl by this reaction. I got A ΔH=-6.55 kJ B.) Calculate ΔH for the formation of 2.80 g of AgCl. C.) Calculate ΔH when 0.110 mmol of AgCl dissolves in water. Need help with B and C.
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=
Given the two reactions PbCl2(s)⇌Pb2+(aq)+2Cl−(aq), K3 = 1.87×10−10, and AgCl(s)⇌Ag+(aq)+Cl−(aq), K4 = 1.18×10−4, what is the equilibrium constant Kfinal for the following reaction? PbCl2(s)+2Ag+(aq)⇌2AgCl(s)+Pb2+(aq)
The solubility product of reaction below at 25C is 1.6x10^-10: AgCl(s) <-> Ag+(aq) + Cl-(aq) show work please and thank you!
Account for your observations. Consider the following equilibria: Ag^+(aq)+Cl^-(aq)<->AgCl(s) Ag^+(aq)+2NH3(aq)<->[Ag(NH3)2]^+(aq) NH3(aq)+H^+(aq)<->NH4^+(aq) Observations: adding NaCl: went from clear to a white solution adding NH3: went from white solution to. clear solution adding HNO3: solution warmed up
Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq) Using the standard free energy of formation values (ΔG⁰f) from the appendix, calculate the Kc value for this reaction. Calculate the ΔG for the dissolving of AgCl in water at 25⁰C when: [Ag+]=[Cl-]= 1.00 x 10-4M