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.
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.
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.
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
The question is: 2. DIIVO U1 QUILD dIl LIC of this experiment. As part of the discussion, explain your results from Part la within the context of Le Châtelier's Principle. Use your observations to help discuss the effect that adding and removing reactants or products has on the position of the equilibrium. The procedure is one of the images and the other image with the test tubes is the results.
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,…
3. Use the following information to answer the next question. Carbon monoxide is an odourless, colourless gas. Carbon monoxide reacts with hydrogen gas to form methane and H2O as CO(g) + 3H2(g) ↔ CH4(g) + H₂O(g). . A chemist pours a mixture of carbon monoxide gas and hydrogen gas in a 500.0 mL reaction vessel in 1:3 ratio. The equilibrium constant for the reaction is 3.92 × 10³, and the equilibrium value of [H2(g)] is 0.21 mol/L. Calculate the equilibrium value of [CO] in mol/L.

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