of 1.00 x10-4 M Ag* and 5.00 x10-5 M Cro42, Ag2CrO4 precipita= of 1.0 x10-4 M Ag* and 1.0 x10-4 M I03", Ag(103) precipitate willf y of Ag2CrO4 is lower than the solubility of Ag(1O3). of 0.200 M CrO42- and 0.200 M 103', Ag2(CrO4) will precipitate ove mixture.
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- Reaction KspKsp ΔH°ΔH° ΔS°ΔS° FeCO3(s)⇄Fe2+(aq)+CO32−(aq)FeCO3(s)⇄Fe2+(aq)+CO32−(aq) 3×10−113×10−11 <0<0 >0>0 MnCO3(s)⇄Mn2+(aq)+CO32−(aq)MnCO3(s)⇄Mn2+(aq)+CO32−(aq) 2×10−112×10−11 <0<0 >0 The table above lists the equilibrium constants and changes in thermodynamic properties for the dissolution of FeCO3 and MnCO3 at 25°C. The two-particle diagrams below represent saturated solutions of each compound at equilibrium. (see attached image) a.) The particle diagrams best represent that ΔH°<0ΔH°<0 because the ions from both compounds are solvated by water molecules. b.) The particle diagrams best represent that ΔH°<0ΔH°<0 because both compounds produce about the same amount of CO32−CO32− ions from the dissolution. c.) The particle diagrams best represent that ΔS°>0ΔS°>0 because both compounds produce a very small amount of ions from the dissolution. d.) The particle diagrams best represent that the molar solubility is greater for…Saturated solution of Fe2S3 is made by dissolving solid compound in water. If [Fe3+] =2.50 x 10-8, calculate the Ksp of Fe2S3.The standard free energy change for the dissolution of Ag₂SO₄ at 25 °C is +28.1 kJ. What is the Ksp of Ag₂SO₄?
- Calculate the Free Gibb’s energy, kJ/mol, for a saturated solution of CdCO3 at 25.0°C. Ksp = 5.2 x 10-12Calculate ΔG'° for a reaction proceeding under biochemical standard conditions with a K'eq of 2.32. Give your answer in units of kJ/mol, but do not include the units as part of your answer (give the number only)Calculate the standard state AG for the following coupled reactions: A> B K'eq= 1.5 X 10S ×+Y= XY K'eq= 1.5 X 10-4 B+x+Y-A+XY AGO= ????
- Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07What is the thermodynamic potential and free energy change of the following reaction Cu/Cu2+(0.0300M)//Ag+(0.0300M)/AgAg+ + e Ag(s) E0 = 0.799 VCu2+ + 2e Cu(s) E0 = 0.337 VCalculate Ksp for the ff. substances, given the molar concentration of their saturated solution. a. Ag2C2O4 ( S= 2.06 x 10-4 ) b. Al(OH)3 ( S = 1.82 x 10-9 )
- The table below provides data for the enthalpy and entropy of formation of compounds A and B at standard conditions (298 K) Compound DHfo (kJ mol-1) Sfo(J K-1mol-1) A –135.2 189.2 B –157.6 192.1 (b) A reversible isomerization reaction converts reactant A to product X. Calculate the Gibbs energy change at non-standard conditions (310 K) if the concentration of A is 2 x 10-4M and that of X is 3 x 10-6 M. Comment on whether the reaction is spontaneous at these conditions. The equilibrium constant Keq = 0.05. Assume standard temperature is 298K.Rose was studying the electric field effect on bacterial growth when he unknowingly carried out an anodic reaction on the platinum electrode that led to the discovery of the anticancer drug cisplatin, cis-[PtCl2(NH3)2]. > Determine the formation constant (Kf) of cisplatin at 25 °C.The Ksp of PbCl2 is 1.7x10-5 at 25oC. What is DGo? Is it possible to prepare a solution that contains Pb2+(aq) and Cl2(aq), at their standard-state concentrations?