Answered: If ΔHsoln < 0, will the conditions for…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 45A

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Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
5.49. Consider the following equilibrium: What is the effect on the equilibrium of each of the following changes? (You may need to calculate some standard enthalpy or Gibbs energy changes to answer these.) (a) The pressure is increased by decreasing the volume. (b) The temperature is decreased. (c) The pressure is increased by the addition of nitrogen gas, .
The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
Determine the equilibrium constant for the reaction Sn+Pb2+Sn2++Pb
In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)
To obtain a precipitate which is useful for gravimetric analysis, the analyst tries to obtain conditions to encourage crystal growth, as opposed to the formation of a colloid. Which of the following statements aids in the formation of a crystalline precipitate and the formation of a colloidal precipitate? Drag your answers to the appropriate markers. (a) The solutions are made as dilute as practical to allow crystals to form slowly. (b) The addition of strong electrolytes (e.g. NaCl or HCl) in the analyte solution, prior to the precipitation reaction. (c) After the digestion of the precipitate, the hot solution is cooled down to room temperature gradually and kept undisturbed overnight. (d) The analyst selects the precipitate of the analyte with the Ksp less than 1 x 10 -15 (e) The Relative Supersaturation value of the analyte solution should be greater than 1 million upon the addition of the precipitating reagent. formation of colloidal precipitate favored formation of crystalline…
Select the reaction for which K, = Kc. 2 Na,0,(s) + 2 CO,(g) =2 Na,CO3(s) + 0,(g) 2 KCIO3 (s) = 2 KCI(s) + 30,(g) 2 H,S(g) + SO,(g)= 3 S(s) + 2 H,O(g) Br, (g) + Cl,(g) 2 BRCI(g)
Write the equilibrium-constant expression Kc for H2(g) + I2(g) => 2 HI(g)
The proper equilibrium expression (Keq) of CH4(g) + 202(g) CO2(g) + 2H2O1).
(a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/L
6 of 12 Part A I Review | Constants Periodic Table Determine the value of the equilibrium constant, Kgoal, for the reaction CO2(g) = C(s) + O2(g), Kgoal =? by making use of the following information: 1. 2CO2(g) + 2H2O(1) = CH;COOH(1) + 202(g), K = 5.40 x 10-16 2. 2H2 (g) + O2(g) = 2H,0(1), K2 1.06 x 1010 3. CH3COOH(1) = 2C(s) + 2H2(g) + O2(g), K3 = 2.68 x 10-9 Express your answer numerically. • View Available Hint(s) 中。 goal = 5:08 AM 19 3/1/2021

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If ΔHsoln < 0, will the conditions for solubility always be met?