Given the two reactions PbCl2(aq)⇌Pb2+(aq)+2Cl−(aq), PbCl2(aq)⇌Pb2+(aq)+2Cl−(aq), K3 = 1.72×10−10, and AgCl(aq)⇌Ag+(aq)+Cl−(aq), AgCl(aq)⇌Ag+(aq)+Cl−(aq), K4 = 1.18×10−4, what is the equilibrium constant KfinalKfinalK_final for the following reaction? PbCl2(aq)+2Ag+(aq)⇌2AgCl(aq)+Pb2+(aq) Express your answer numerically.

Given the two reactions PbCl2(aq)⇌Pb2+(aq)+2Cl−(aq), PbCl2(aq)⇌Pb2+(aq)+2Cl−(aq), K3 = 1.72×10−10, and AgCl(aq)⇌Ag+(aq)+Cl−(aq), AgCl(aq)⇌Ag+(aq)+Cl−(aq), K4 = 1.18×10−4, what is the equilibrium constant KfinalKfinalK_final for the following reaction? PbCl2(aq)+2Ag+(aq)⇌2AgCl(aq)+Pb2+(aq) Express 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

The following gaseous system is in equilibrium at 30.00C and 1 bar, where 25% of N2O4 is dissociated into NO2: N2O4(g) 2 NO2(g) (a) Calculate the equilibrium constant, K. (b) Calculate the extent of the dissociation, a at 30.00C and 0.1 bar.
Silver chloride can be formed from metallic silver and hydrogen chloride, based on the reaction: 2 Ag (s) + 2 HCl (g) 2 AgCl (s) + H2 (g) The Gibbs function for the formation, at 25ºC, are the following: For HCl(g) is -95.3 kJ mol-1 and for AgCl(s) is -109.7 kJ mol-1 a) Knowing the reaction constant K = 1.5·103 at 80 ºC, Find the average enthalpy of reaction, considering constant in the range of 0 to 150 ºC. b) Assuming that the gases behave ideally, find the temperature at which, 90% of HCl has reacted at a total pressure of 0.05 atm when it reaches the equilibrium.
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
For the hypothetical reaction 2A(g) + B(g) ⇌ 3C(g) + heat, the equilibrium constant is 0.138 at 45∞C. What is the equilibrium constant for reaction, 3C(g) + heat ⇌ 2A(g) + B(g)?
Stearic acid dimerizes when dissolved in carbon tetrachloride, CCl4: 2 C17H35COOOH-------------------------- à (C17H35COOH)2 The equilibrium constant, Keq, is 2780 at 22°C but dr0ps to 93.1 at 42°C. From this information, estimate ∆H° and ∆S°.
For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard Gibbs free enthalpy change is 1.62 kJ at 25oC. The initial concentration of A(aq) is 0.562 M, the initial concentration of B(aq) is 0.335 M, and the initial concentration of C(aq) is 0.202 M. What would be the concentration of A(aq) (in mol/L) once we attain equilibrium (we are still at 25oC)?
A mixture of gaseous CO and H2, called synthesis gas, is used commercially to prepare methanol (CH3OH), a compound considered an alternative fuel to gasoline. Under equilibrium conditions at 570.3 K, [H2] = 0.06302 mol/L, [CO] = 0.03125 mol/L, and [CH3OH] = 0.0401 mol/L. What is the value of Kc for this reaction at 570.3 K?
assuming the volume is 1 dm3, calculate the equilibrium constant for the reaction of A2+ 2A (g) >2AB(g) If the volume of the equilibrium mixtures is decreased, will the number AB molecules increase or decrease and why
For the following reactionC(??) + 2H2(??) ⇌ CH4(??)K =0.26 at 1000 °C (3 significant figures). What is the equilibrium constant at 750 °C (3significant figures)?
Consider the reaction scheme for degradation of water 1 atm: Reaction 1: H2O ↔ H2 + 1/2 O2 Reaction 2: H20 ↔ 1/2 H2 + OH Delta G1 = 228,566 kJ/kmol Delta G2 = 263.270 kJ/kmol AHr1° = 241,820 kJ/kmol AHr2° = 281,280 kJ/kmol A) Calculate the value of the equilibrium constant for each Reaction at 25°C. What does this tell you about the equilibrium composition B) Estimate the equilibrium constant for each reaction 1 at 5,000°C. C) Fully set up and explain how you would solve for the equilibrium composition of reaction mixture which started with 1 mole of water. Include an expression for the equilibrium constant(s) in terms of composition as part of your answer.
The equilibrium constant for the reaction 2Fe3+(aq) + Hg22+(aq) ⇌ 2Fe2+(aq) + 2Hg2+(aq)is Kc = 9.1 x 10-6 at 298 K.(a) What is ΔG° at this temperature?(b) If standard-state concentrations of the reactants and products are mixed, in which direction does the reaction proceed?(c) Calculate ΔG when [Fe3+] = 0.20 M, [Hg22+] = 0.010 M, [Fe2+] 5 0.010 M, and [Hg2+] 5 0.025 M. In which direction will the reaction proceed to achieve equilibrium?
Consider the following reaction:CH3OH(g) CH2O(g) + H2(g) K = 3.29 x 10−11a. If 14.4 g of CH3OH(g) is added to a 1.50 L container at 298 K, calculate the equilibriumconcentrations of all gases b. Without doing any calculations, predict what happens if the reaction is put in a 2.00 Lcontainer instead of a 1.50 L container. c. . Without doing any calculations, predict what happens if H2SO4 (a catalyst) is added