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…

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem 17STP

See similar textbooks

Similar questions

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.
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Kc1,1, or 1 for a titration reaction?
Would either of the following reactions go almost completely to product at equilibrium? a 2NO(g)+2H2(g)N2(g)+2H2O(g);Kc=6.510113 b COCl2(g)CO(g)+Cl2(g);Kc=361016
The labels on most pharmaceuticals state that the medicine should be stored in a cool, dark place. In the context of this chapter, explain why this is sound advice.
. 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.
s) Consider the following reaction at equilibrium. State the effect that each of the following would have on equilibrium H₂CO(g) →H*(aq) + HCO₂ (aq) a) adding NaHCO₂ b) increasing T c) Adding NaOH AH<0
Kinetics and Equilibrium Calculating an equilibrium constant from a heterogeneous equilibrium... Try Again Try again... Bis 2/5 Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. Fluoride anion and hydronium cation react to form hydrofluoric acid and water, like this: F (aq)+H3O (aq)→HF (aq) + H2O(l) At a certain temperature, a chemist finds that a 9.9 L reaction vessel containing an aqueous solution of fluoride anion, hydronium cation, hydrofluoric acid, and water at equilibrium has the following composition: compound amount F 0.146 g H₂O 0.364 g HF 4.96 g 892. g H₂O Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K 8.4 x 10 C
Use the reaction system below to answer the questions that follow. Predict the effect of changes in each question on the position of equilibrium. HNO2 (aq) + H2O(l) ⇌ H3O+(aq) + NO2-(aq) Increasing the pH... I. Shifts to the products. II. Shifts to the reactants III. No change in equilibrium position. because… IV. the chemical species is not in the equilibrium expression. V. decreasing the concentration of reactants increases the rate of the reverse reaction. VI. decreasing the concentration of products increases the rate of the forward reaction.
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,…
No need for solutions, just the correct answers. Thank you!
Relative Concentrations at Equilibrium (two parts) Reactant A undergoes dissociation into products B and C according to the following equilibrium reaction equation A(g) = B(g) + C(g) A rigid vessel, initially containing 0.076 mol/L of pure A, is allowed to equilibrate at 53°C. What would be the value of the equilibrium constant (Keg expressed in terms of the molar concentrations) if the equilibrium concentrations of all species are equal? (No units required.)

SEE MORE QUESTIONS

Recommended textbooks for you

Living by Chemistry

Chemistry

ISBN:

9781464142314

Author:

Angelica M. Stacy

Publisher:

W. H. Freeman

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Living by Chemistry

Chemistry

ISBN:

9781464142314

Author:

Angelica M. Stacy

Publisher:

W. H. Freeman

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Chemistry for Engineering Students

Chemistry

ISBN:

9781285199023

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS