Express the equilibrium constant for the following reaction: 2 CH2CI2 (9) + Clz (9) 32 СHC\з + H2 () [CHCI;]!/?{H2] k = [CHCI3J°[H2] k = [CHCI,}[C1,] [CHCI,I°ICI;] k = [CHCI3]°[H2] [CHCI,ICI2] k = [CHCI3][H2] [CHCI3][H2] k = [CHCI,[Cl,]
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![Express the equilibrium constant for the following reaction:
2 CH2CI2 (9) + Clz (9) 32 СHC\з + H2 ()
[CHCI;]!/?{H2]
k =
[CHCI3J°[H2]
k =
[CHCI,}[C1,]
[CHCI,I°ICI;]
k =
[CHCI3]°[H2]
[CHCI,ICI2]
k =
[CHCI3][H2]
[CHCI3][H2]
k =
[CHCI,ICI2]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe74f1f16-fe05-4c3f-a6b1-b72493415d70%2F38cb7151-b948-4ed2-970c-f2f325464f42%2F0y68qy_processed.png&w=3840&q=75)
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- Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.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 = 32.07Hexanoic acid was added to an immiscible biphasic solvent system, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D2) of hexanoic acid in water with respect to CCl4.
- One litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?Given that the Ksp for Ag2S is 6×10^-51, Kf=1.1×10^5 for AgCl2-, and Ka1 and Ka2 for H2S are 9.5×10^-8 and 1×10^-19, respectively, calculate the equilibrium constant for the following reaction .Consider the reaction CaCl2 (s) = Ca2+ (g) + 2Cl- (aq) (Ksp = 5.5 x 10-6) 1. What is the solubility (in mg/L) of calcium chloride at 298K? 2. What is the equilibrium concentration of chloride ions in a saturated solution of calcium chloride? 3. What is the pH of this solution?
- The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq) which is a common ion then what would be the concentration of the Arsenate ion AsO43-(aq) in Molarity at equilibrium? 1.97 x 10-2 2.78 x 10-2 2.38 x 10-2 1.74 x 10-2 3.24 x 10-2 2.99 x 10-2 2.57 x 10-2 2.11 x 10-2 1.55 x 10-2 1.35 x 10-2The Ksp of Fe3(PO4)2 is 5.51⋅10-21 M. Calculate the solubility of Fe2+ and PO43- in a saturated solution.Sulfuric acid (H2SO4) is a strong acid in aqueous solution, yet the pKa of sulfuric acid is 7.6 in acetonitrile (CH3CN). Explain how this can be in terms of the relevant equilibria and the properties of the two solvents.
- 1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.To compute the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25 degrees celcius until the solution is saturated. Ba(NO3)2 is only slightly soluble in water. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: ?a(NO3)2(s) ⇄ Ba2+(aq) + 2NO3- (aq) Ksp = [Ba2+][NO3-]2 What is the solubility product Ksp and vapor pressure of the solution?Given the equilibrium constant valuesN2(g)+1/2O2(g)⇌N2O(g) KC=2.7×10−18 N2O4(g)⇌2NO2(g) KC=4.6×10−3 1/2N2(g)+O2(g)⇌NO2(g) KC=4.1×10−9 Determine a value of KC for the reaction: 2N2O(g)+3O2(g)⇌2N2O4(g)