. Generate equilibrium constant expression for the reaction: Tl3++ 2Fe2+↔Tl++ 2Fe3+E°Fe3+= +0.771 V E°Tl+= +1.25 VCalculate the numerical value for Keq
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12. Generate equilibrium constant expression for the reaction: Tl3++ 2Fe2+↔Tl++ 2Fe3+E°Fe3+= +0.771 V E°Tl+= +1.25 VCalculate the numerical value for Keq.
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- For the reaction N2(?) + 3 H2(?) ⇌ 2 NH3(?):a. Write an expression for standard reaction Gibbs energy, ∆rG, in terms of chemical potentials.b. Write an expression for the reaction quotient, Qp, in terms of the partial pressures.c. The equilibrium constant at 25 °C is 5.8 × 10^5. What is the standard reaction Gibbsenergy, ∆rG?Consider the mixing of 25.00 mL of 0.0500 M Pb(NO3)2 with 25.00 mL of 0.0500 M NaCl and the equilibrium reaction, PbCl2(s) ⇌ Pb2+(aq) + 2Cl-(aq) Ksp = 1.20 x 10-5 What is the molar concentration of Pb2+ in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the molar concentration of Cl- in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the ion product (Q)? Will a precipitate form? (yes or no)Express the equilibrium constant for N2O4(g) ⇌ 2 NO2(g) in terms of the fraction a of N2O4 that has dissociated and the total pressure p of the reaction mixture,and show that when the extent of dissociation is small, a ≪1, a is inversely proportional to the square root of the total pressure, a ∝ p-1/2.
- Determine equilibrium constant for the reaction: Fe2+ + Cr2O72- --- Fe3+ + Cr3+ Given: Fe2+ + 2 e --------- Fe (s) Eo = - 0.44 Fe3+ + e ------ Fe2+ Eo = 0.771 V Cr2O72- + 14 H+ + 6 e ------- 2 Cr3+ + 7 H2O(l) Eo = 1.36 V A. 3.15 x 10-60 B. 5.24 x 1059 C. 1.90 x 1093 D. 1.90 x 1060 E. 4.50 x 1050Calculate the value of the reaction quotient, Q, of silver iodate (AgIO3) when 10.0 mL of 0.018 M AgNO3 is mixed with 10.0 mL of 0.018 M NaIO3. (Please give your answer with 2 significant figures.)The equilibrium constant of the reaction 2 C3H6 (g) ⇌ C2H4(g) + C4H8(g) is found to fit the expression InK= -1.04-(1088 K)/T +(1.51 x 10-2 K2)/T2between 300 K and 600 K. (a) Calculate the standard reaction Gibbs energy at each temperature at 390 K and 410 K. (b) Use the van 't Hoff equation to determine the standard reaction enthalpy at 400 K. (c) Hence also calculate the standard reaction entropy at 400 K.
- How can I determine the equilibrium constant at the recorded temperature for the esterification reaction of ethanol and acetic acid? Recorded temp for flask B : 28°CEstimate the equilibrium constant for the system indicated at 25oC. 3 Mg2+ + 2 Al --> 3 Mg + 2 Al3+ A. ~10-36 B. ~1069 C. ~1023 D. ~10-24 E. ~10-72The 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 10-2
- 1. Write the dissociation reaction and solubility product constant expression for the following sparingly soluble salt. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 2. Determine the Molar Solubility of the following sparingly soluble salt in water. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 3. Express the solubility (S) in question #2 in g/L. 4. Calculate Ksp for the ff. substances, given the molar concentration of their saturated solution. a. Ag2C2O4 ( S= 2.06 x 10-4 ) b. Al(OH)3 ( S = 1.82 x 10-9 ) 5. Calculate the molar solubility of the salts in problem #2 for the solution in which the cation concentration is 0.050 M.1. Given the following equilibria and equilibrium constants. Ca2+ + 2C2O42- + H2O <-> CaC2O4•H2O(s) Ksp = 1.96×10-8 H2C2O4 <-> H+ + HC2O4- Ka1 = 5.60×10-2 HC2O4- <-> H+ + C2O42- Ka2 = 5.42×10-5 Which species would increase upon the addition of 0.1 M HCl(aq)? 2. Solid Mn(OH)2(s) is added to 1.0 liter of distilled water. What is the concentration of Mn2+ in the solution? The Ksp for Mn(OH)2(s) is 1.6×10-13. 3. Solid Mn(OH)2(s) is added to 1.0 liter of a 0.01 M NaOH solution. What is the concentration of Mn2+ in the solution? The Ksp for Mn(OH)2(s) is 1.6×10-13. 4. Most sulfide compounds of transition metals are very insoluble. However, the solubility products vary over a wide range and separations of metal sulfides can be accomplished by using the pH of the solution to control the S2- concentration.…It is found that 8.70e-09 g of Ga(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ga(OH)3.The Ksp of Y2(CO3)3 at 25 oC is 1.03e-31. What is the molar solubility of Y2(CO3)3?