! ( give ans with explanation ) Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction:I(aq) + I2(aq) 13 (aq)K = 710.For each of the following cases calculate the equilibrium ratio of [I;] to [I2].7.00x10-2 mol of I, is added to 1.00 L of 7.00x10-1 M KI solution.Submit Answer Tries 0/5The solution above is diluted to 13.00 L.

Answered: Image /qna-images/answer/1b5f55fd-3aa1-4301-a492-24aebc5af186.jpg

Iodine is sparingly soluble in pure water. However, it does dissolve' in solutions containing excess iodide ion because of the following reaction: (be) EI = (be)čI + (be).I K = 710. For each of the following cases calculate the equilibrium ratio of [I3] to [12]. 7.00x10-2 mol of I2 is added to 1.00 L of 7.00x10-1 M KI solution. Submit Answer Tries 0/5 The solution above is diluted to 13.00 L.

Iodine is sparingly soluble in pure water. However, it does dissolve' in solutions containing excess iodide ion because of the following reaction: (be) EI = (be)čI + (be).I K = 710. For each of the following cases calculate the equilibrium ratio of [I3] to [12]. 7.00x10-2 mol of I2 is added to 1.00 L of 7.00x10-1 M KI solution. Submit Answer Tries 0/5 The solution above is diluted to 13.00 L.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section15.6: Disturbing A Chemical Equilibrium

Problem 2.3ACP: A 0.64 g sample of the white crystalline dimer (4) is dissolved in 25.0 mL of benzene at 20 C. Use...

See similar textbooks

Similar questions

The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Write the expression of the reaction quotient for the ionization of HOCN in water.
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)