E 4 4 Calculate for the process for the reaction: Ag:AsO4(s)+3e 3Ag(s) +AsO Ksp for AgAsO4...
o. Study this chemical reaction: ups ni sorlg dst noitos ollat 3AGNO3(aq) + Al(s) 3Ag(s) +Al(NO3)3(aq) 09:6h) Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction. 31 Oxidation: A Al 3e Aate Reduction: Ag
F1. What is the Koverall given the information below: Ag3AsO4 (s) < > 3 Ag+ (aq) + AsO 3- (aq) Agt (aq) + 2 NH; (aq) <- > Ag(NH3)2(aq) AgAsO4(s) + NH3(aq) <_> 3Ag(NH3)2 (aq) +AsO?"(aq) Ksp=1.0 x 10-22 Ki-1.6 x 107 Koverall = ???
Calculate E°cell for a silver-aluminum cell in which the cell reaction is?Al(s) + 3Ag+(aq) ? Al3+(aq) + 3Ag(s)A. -2.46 V B. 0.86 V C. -0.86 V D. 2.46 V E. none of these
a) Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its molar solubility. b) If Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its mass solubility in g solute/100g of water. Please answer a & b
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.
The solubility of AgCN (s) in 0.200M NH3 (aq) is 8.8×10−6mol/L. Calculate Ksp for AgCN. ANSWER Ksp = 1.2×10−16
Calculate the molar solubility of: a. ZnC2O4 Ksp = 2.70 x 10-8 e. PbCO3 Ksp = 7.39 x 10-14 b. Ag2S Ksp = 6.00 x 10-51 f. Al(OH)3 Ksp = 1.81 x 10-5 c. BaCrO4 Ksp = 1.22 x 10-10 g. CaF2 Ksp = 5.29 x 10-9 d. Mg3(PO4)2 Ksp = 1.01 x 10-25 h. Fe4[Fe(CN)6]3 Ksp = 3.34 x 10-41
at 298 K For the reaction: 2NO2 (g)N2s (e) The value of AHo and Aso are-58.03 kJ and -176.6 J/K, respectively (a) What is the value of AG at 298 K? (b) At what temperature would this process be spontaneous?
calculate the initial pH of the solution given the following reaction. Ca(OH)2 -> Ca2+ + 2OH- with ksp= 1.3 x 10^-6 please explain how you got your answer. 15) (5 pts) Calculate the initial pH of the solution given the following reaction and equilibrium information below: Ca(OH),(s) = Ca2+ (aq) + 20H- (aq) with Ksp = 1.3 x 10-6 A) 8.2 B) 10.3 C) 11.8 D) 12.1 E) None of these are correct + Ann
Given the Ksp = 1.2 x 10-12 for Ag2 CrO4 and K+ = 1.7 x 107 for (Ag(NH3)21, calculate the equilibrium constant for Ag2CrO4(s) + 4 NH3(aq) + 2 Ag(NH3)21+ (aq) + Cr042-aq) and explain whether the reaction favors reactants or products at equilibrium? Show work. TTT Arial 3 (12pt) • T. E. 3. 's Path:p Words:0