The following equilibrium constants have been determined for hydrosulfuric acid at 25°C9.5x108H(aq)HS (aq)(aq)H25(aq)Kc" - 1.0x10 19s (aq)HS (aq)+.H(aq)Calculate the equilibrium constant Kc for the following reaction at the same temperature.s²2H(aq)(aq)+.H2S aq)a.18x10-18Obg 5y10-27-3.4x10-163.78x104>Oe19x10-24

Answered: Image /qna-images/answer/b2bf69c9-6ba5-4d9a-925b-1bcb93a87031.jpg

The following equilibrium constants have been determined for hydrosulfuric acid at 25°C; HS (aq) Kc = 9.5x108 H2S(aq) H* (aq) s2 (ag) Kc = 1.0x10-19 HS (aq) H (aq) Calculate the equilibrium constant Kc for the following reaction at the same temperature. 2H (aq) s2 (aq) +. H2S(aq) O a.18x10 18 Ob.g 5x10-27 OC.3.4x10-16 O d.7.8x10-25 O e.19x10-24

The following equilibrium constants have been determined for hydrosulfuric acid at 25°C; HS (aq) Kc = 9.5x108 H2S(aq) H* (aq) s2 (ag) Kc = 1.0x10-19 HS (aq) H (aq) Calculate the equilibrium constant Kc for the following reaction at the same temperature. 2H (aq) s2 (aq) +. H2S(aq) O a.18x10 18 Ob.g 5x10-27 OC.3.4x10-16 O d.7.8x10-25 O e.19x10-24

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 70AP

See similar textbooks

Similar questions

Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C
Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
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, .
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
5.11. Determine the numerical value of Q for the reaction conditions indicated.
Which of the following reactions in equilibrium can be affected by changes in pressure? AgCI(s) = Ag*(aq) + Cl¯(aq) a. b. SO;(g) + H,O(/) = H,SO,(aq) P,O106) + 6H,O(I) = 4H,PO,(aq) CH,COOH(aq) = CH,COO (aq) + H*(aq) с. d. (DO1
Consider the reaction at 25 degrees celsius 2NO3-(aq)+8H^+(aq)+3Cu(s)=3Cu2+(aq)+2NO(g)+4H2O(l) At what pH is the reaction at equilibrium with all other ionic species at 0.01M and gases at 1 atm?