11. Given the reaction below, answer the following questions:Br +KIacetoneAa) Based on the equation above and knowing that an excess of potassium iodide is used, wouldyou expect this reaction to be favorable? Please explain.b) This is a reaction commonly employed in organic chemistry and takes several hours of heatingthe mixture at reflux for the reaction to go to completion. During the course of the reaction acrystalline precipitate forms. What is the precipitate?Why does this provide thedriving force for the reaction?c) In general this reaction is not used in practice to convert optically active secondary alkylbromides to optically active alkyl iodides because the alkyl iodide products tend to lose opticalactivity if the reactions are run too long or if too much potassium iodide is used. Pleaseexplain.

a) This reaction involves the nucleophilic substitution of an alkyl bromide with potassium iodide in…

Answered: 11. Given the reaction below, answer…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section14.1: Bronsted-lowry Acids And Bases

Problem 14.2CE: Using Le Chatelier’s Principle Use Le Chatelier’s principle (← Sec. 12-6b) to explain why the...

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Complete the changes in concentrations for each of the following reactions: (a) AgI(s)Ag+(aq)+I(aq)x (b) CaCO3(s)Ca2+(aq)+CO32(aq)x (c) Mg3(OH)2(s)Mg2+(aq)+2OH(aq)x (d) Mg3( PO4)2(s)3Mg2+(aq)+2PO43(aq)x (e) Ca5( PO4)3OH(s)OH(s)5Ca2+(aq)+3PO43(aq)+OH(aq)x
Describe any thermochemical (heat of reaction) evidence for the Arrhenius concept.
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. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
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I Review | Constants | Periodic Table Part B When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K. The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: The following system is at equilibrium:A(s) + 4B(g) = C(g)Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help If a stress is applied to a reaction mixture at equilibrium,…
14:52 Wed Feb 17 * 75% T O + : Name: Date: EXPERIMENT 2 QUALITATIVE CATION ANALYSIS PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to introduce you to several ideas that are important to aspects of the experiment. You must turn in your work to your instructor before you will be allowed to begin the experiment. 1. Complete the following solubility table. (Simply enter S for soluble or I for insoluble in each cell). NO3 SO2- CO3²- Cl Li* Ag* I Cu2+ Sr+ 2. Write net ionic equations for those combinations that produce insoluble products. Co 1 3 СHM 1024 — Ехрeriment 2. Qualitative Cation Analysis Page 1 of 2

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