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18. If the Ksp for a compound dissolving in water at 25°C is 2.4. Determine AG...
Which is the correct Ksp expression for Ag2CrO4 (s) dissolving in water? Ksp = [Ag*12(CrO42-1 Ksp = (Ag*12[Cr3+][02-14 Ksp = [A8+][Cro_2-12 Ksp - [Ag*][Cro42-1
For the Dissolving of PbCl2 in water Ksp is 1.7 x 10^-5. calculate deltaG standard at 25 degrees C. 12. For the dissolving of PbCl2 in water Ksp is 1.7 x 10-5. Calculate AG at 25°C. If [Pb2+] = .010M and [Cl-) = .01M what is AG?
Determine the molar solubility and value of Ksp for each compound in water at 25°C. Include the chemical equation for each equilibrium, the expression for Ksp (in terms of molarities and x), and show all work in calculations Compound 1: SrSO4 Compound 2: Ag2SO4 Chemical equation: Molar solubility (x) = Ksp =
Based on the ∆Go = -RTlnK expression, would you predict that AgCl (s) dissolving into Ag+ (aq) and Cl- (aq) (Ksp = 1.8x10-10) is a spontaneous process? Yes or no. I am having a hard time grasping this concept, so could you show your work please? Thank you :)
AG°= AH-TAS AG=AGº+RTinQ where R=8.314 J/mol K 1. Calculate AGº for the following reaction at 25 °C if AH°= -1854 kJ/mol; AS°= -236 J/mol K CH-COCH3(g) + 402(g) → 3C02(g) + 3H2O(1) 2. NH.NO, dissolving in water is a spontaneous process. As it dissolves, the temperature of the solution decreases. Based on this, what must the signs (positive or negative) of AG, AH, and AS be?
A saturated solution is prepared by dissolving Al(OH)3 (Ksp = 2*10^-32) in pure water at 25 C. Which of the following could to add to the solution to dissolve more Al(OH)3? A. Ar B. KCl C. HBr D. NaOH E. NH3 NOTE: I know the answer is C, I need the reasoning to get there.
5. Based on the AGⓇ =-RT In K expression, would you predict that AgCl(s) dissolving into Ag+ (aq) + CI+ (aq) [Ksp = 1.8x10-1') is a spontaneous process? Would you expect Co3+ (aq) +6NH3(aq) forming the [CO(NH3)6]+ complex ion [Kp = 4.5x1033] to be a spontaneous process? How does the magnitude of the equi- librium constant relate to the AGº? If a saturated solution of calcium hydroxide is prepared and its Ksp is determined, how can the AG = AGº+RT...
* 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!
Calculate the solubility of Ag2CrO4 in water at 25°C. You'll find Ksp data in the ALEKS Data tab. Round your answer to 2 significant digits. (Ksp=1.12x10^-12) Calculate the solubility of Ag, CrO4 in water at 25 °C. You'll find K data in the ALEKS Data tab. Round your answer to 2 significant digits. Flora x 6 ?
Chapter 18 Thermodynamics Homework 1.Predict the sign of AS for each process: a) The boiling of water b)2HgO(s)-2Hg(I) + 02(s) c) CaCO, (s)CaO(s)+ CO (g) 2. Is the following process spontaneous or nonspontaneous at a given temperature? NaNO,(s) ->NaNO,(aq) 3. If a reaction has ΔS < 0 and ΔΗ < 0 will the reaction always be spontaneous, spontaneous at low T, spontaneous at high T, or never spontaneous? 4.Consider this reaction: Calculate ΔG at 25 °C and determine whether the...