please help thanks Calculate Ksp for the salt NaCl at 25°C. Substance Na+(aq) Cl'(aq) NaCl(s) DGfº(in kJ/mol) -2620...
please help thanks Calculate Ksp for the salt NaCI at 25°C. Substance DG (in kJ/mol) Na (aq) 2620 Cl (aq) -131.0 NaCl(s) -383.8 4.1 41 1.7 1019 0.41 9.2
NaCl(s) ⇌ Na+(aq) + Cl-(aq) ΔHo = 3.9 kJ/mol At 298 K, a saturated solution of NaCl has [Na+] = 7.0 M and [Cl-] = 5.4 M. If the temperature of the mixture is increased to 323 K, what will be the equilibrium concentration (M) of Na+? (Assume no ion pairing.) Enter your answer to 2 decimal places. NaCl(s) Na (aq) + CI'(aq) AH- 3.9 kJ/mol At 298 K, a saturated solution of NaCI has [Na"] 7.0M and [CI] -...
calculate the lattice energy of NaCl based on the given information : ΔH°f[NaCl(s)] = -411 kJ/mol ΔH°f [Clg] = 121.5 kJ/mol ΔH°sublimation [Na] = 109 kJ/mol IE1 (Na) = 496 kJ/mol EA1 (Cl) = -349 kJ/mol
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 =
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=
The salt ammonium chloride dissolves in water according to the reaction: NH4Cl(s) NH4+(aq) + Cl-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: NH4Cl(s) = -314.4 kJ mol-1 NH4+(aq) = -132.5 kJ mol-1 Cl-(aq) = -167.2 kJ mol-1 kJ (b) Calculate the temperature reached by the solution formed when 35.3 g of NH4Cl is dissolved in 0.160 L of water at 24.6 °C. Approximate the heat capacity of the solution by the heat capacity...
< Question 13 of 18 > Consider the Gibbs energies at 25 °C. Substance AG (kJ. mol-!) Ag+ (aq) 77.1 Cl(aq) -131.2 AgCl(s) -109.8 Br" (aq) -104.0 AgBr(s) -96.9 (a) Calculate AGran for the dissolution of AgCl(s). kJ. mol- (b) Calculate the solubility-product constant of AgCl. kJ. mol- (b) Calculate the solubility product constant of AgCl. K = Enter numeric value (c) Calculate AGtx for the dissolution of AgBr(s). kl. mol-? (d) Calculate the solubility-product constant of AgBr. K=
Assuming that the solubility of PbBr2(s) is 2.1x10 mol/L at 25°C, calculate the Ksp for this salt. Ignore any potential reactions of the ions with water.
Thermodynamic Quantities for Selected Substances at 298 15K (25 °C) Substance AHºt (kJ/mol AG' (kJ/mol) SOK-mol) Calaum Ca(s) CaCl2 (s) Ca2+ (aq) 0 -795.8 0 -748.1 41.4 104.6 200.8 226.7 209.2 Chlorine Cl2 (8) Cl- (aq) 0 0 222 96 565 -167 2 -131.2 Oxygen 02 (8) H20 (1) 0 -285.83 -237 13 69.91 Phosphorus P2 (8) PC13 (8) POCl3 (8) 144.3 -2881 -5422 103.7 -269.6 -502.5 2181 3117 325 Sulfur S (s, rhombic) 90 268) 903(8) 0 -2699 -395.2...
A generic salt, AB,, has a molar mass of 333 g/mol and a solubility of 2.40 g/L at 25 °C AB2 (s) A(aq) 2B (aq) What is the Ksp of this salt at 25 °C? Ksp