Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), H2S(aq)⇌HS−(aq)+H+(aq), K1K1K_1 = 9.78×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), HS−(aq)⇌S2−(aq)+H+(aq), K2K2K_2 = 1.43×10−19, what is the equilibrium constant KfinalKfinalK_final for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq)S2−(aq)+2H+(aq)⇌H2S(aq) Enter your answer numerically.

Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), H2S(aq)⇌HS−(aq)+H+(aq), K1K1K_1 = 9.78×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), HS−(aq)⇌S2−(aq)+H+(aq), K2K2K_2 = 1.43×10−19, what is the equilibrium constant KfinalKfinalK_final for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq)S2−(aq)+2H+(aq)⇌H2S(aq) Enter your answer numerically.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 81QAP

See similar textbooks

Similar questions

Given the following two equilibria at 750 K. NiCO3 (s) ⇔ Ni2+(aq) + CO32-(aq) Kc = 6.6 x 10-9 HCO3- (aq) + H2O(liq.) ⇔ CO32- (aq) + H3O+ (aq) Kc = 4.8 x 10-11 Based on the above two equilibria, calculate the equilibrium constant for the following reaction at 750 K. NiCO3(s) + H3O+ (aq) ⇔ Ni2+(aq) + HCO3- (aq) + H2O(liq.
A solution of 89.1 ml of 0.00185 M A1B3 is mixed with a solution of 49.44 ml of 0.00800 M C1D3. Find the value of pQ (the minus log of Q) for the formation of C1B3.
Write the equilibrium-constant expressions and obtain numerical values for each constant ina. the basic dissociation of ethyl amine, C2H5NH2.b. the acidic dissociation of hydrogen cyanide, HCN.c. the acidic dissociation of pyridine hydrochloride, C5H5NHCl.
Use data from Appendix IIB to calculate ΔS∘rxnΔSrxn∘ for each of the reactions given. 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g) Express your answer as an integer. ΔS∘rxn=____________________J/K
Determine the equilibrium constant for the reaction below using the following information: 2 JQ ⇌ J2 + Q2 KC = 0.28 3.5 J2 + 3.5 Q2 ⇌ 7 JQ KC = ? Group of answer choices -0.98 171 13 -0.012 86
Write the equilibrium-constant expressions and obtain numerical values for each constant in the acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl. the dissociation of H3AsO3 to H3O+ and AsO33-
What is true of ΔG'° when K'eq is 0.5? Select one - Negative - Zero - Positive - There isn't a relationship between ΔG'° and K'eq
Calculate the equilibrium constant at 25.0 oC for the following equation. Cr2O7-2(aq) + 6Fe+2(aq) + 14H+1(aq) ↔2Cr+3(aq) + 6Fe+3(aq) + 7H2O(l) Group of answer choices 1.46x1010 6.34x1046 2.52x1023 1.58x10-47
For the equilibrium: A ↔ B, if [A]o = 0.162, [B]o = 0.569, and Keq = 47.8, what are [A]eq and [B]eq? Only show the algebraic expression with final [A]eq and [B]eq
Calculate the equilibrium constant k for the following reaction at 84 degree C A2 + B2 > 2AB Given Delta H(kJ/mol) DeltaS(J/mol K) A2 0 122 B2 0 -105 AB -40 278 Write your answer in exponential form
You have found the following: CaSO4(s) <=> Ca+2(aq) + SO4-2(aq) K = (6.053x10^-5) What is the value of K for the following reaction? 2 CaSO4(s) <=> 2 Ca+2(aq) + 2 SO4-2(aq) Note: Your answer is assumed to be reduced to the highest power possible. Please provide neat and clean handwriting and clear image Give answer correctly
The following equilibrium constants have been determined for hydrosulfuric acid at 25ºC: H2S(aq) ⇌ H+(aq) + HS–(aq) K′c = 9.5 × 10–8 HS–(aq) ⇌ H+(aq) + S2–(aq) K″c = 1.0 × 10–19 Calculate the equilibrium constant for the following reaction at the same temperature. H2S(aq) ⇌ 2H+(aq) + S2–(aq)