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
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Blood pH can be impacted by the carbonic acid/bicarbonate system, which utilizes the following formula: CO2 + H2O << H2CO3 « HCO3 + H* What effect would the IV bicarbonate have on the carbonic acid/bicarbonate reaction above? Shift it to the left B Shift it to the right (C) Settle it closer to equilibrium No effect.
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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,…
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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.)

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