පිපිම Draw curved arrows to represent the flow of electrons in the reaction on the left Label the reactants on the left as either "Acid" or "Base" (iii) Decide which direction the equilibrium arrows will point in each reaction, based on the given pk, values (a) + H-O H 3-H + (c) H" H + H****H 000 44-00 NH₂ (e) i Дон OH Ө NH

පිපිම Draw curved arrows to represent the flow of electrons in the reaction on the left Label the reactants on the left as either "Acid" or "Base" (iii) Decide which direction the equilibrium arrows will point in each reaction, based on the given pk, values (a) + H-O H 3-H + (c) H" H + H****H 000 44-00 NH₂ (e) i Дон OH Ө NH

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter7: Reaction Rates And Chemical Equilibrium

Section: Chapter Questions

Problem 7.20P

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7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
7-41 The equilibrium constant at 1127°C for the following endothermic reaction is 571: If the mixture is at equilibrium, what happens to K if we: (a) Add some H2S? (b) Add some H2? (c) Lower the temperature to 1000°C?
Suppose a reaction has the equilibrium constant K = 1.7 108 at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?
7-71 You have a beaker that contains solid silver chloride (AgCl) and a saturated solution of Ag+ and CI- ions in equilibrium with the solid. You add several drops of a sodium chloride solution. What happens to the concentration of silver ions?
7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
Le Chteliers principle is stated (Section 12-7) as follows: If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change. The systemN2(g)+3H2(g)2NH3(g) is used as an example in which the addition of nitrogen gas at equilibrium results in a decrease in H2 concentration and an increase in NH3, concentration. In the experiment the volume is assumed to be constant. On the other hand, if N2 is added to the reaction system in a container with a piston so that the pressure can be held constant, the amount o f NH3 actually could decrease, and the concentration of H2 would increase as equilibrium is reestablished. Explain how this can happen. Also, if you consider this same system at equilibrium, the addition of an inert gas. holding the pressure constant, does affect the equilibrium position. Explain why the addition of an inert gas to this system in a rigid container does not affect the equilibrium position.
7-32 A particular reaction has an equilibrium constant of 1.13 under one set of conditions and an equilibrium constant of 1.72 under a different set of conditions. Which conditions would be more advantageous in an industrial process that sought to obtain the maximum amount of products? Explain.
Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: CH3CO2HAceticacid+C2H5OHEthanolCH3CO2C2H5Ethylacetate+H2OK=2.2 For the following mixtures (a-d), will the concentration of H2O increase, decrease, or remain the same as equilibrium is established? a. [CH3CO2C2H5] = 0.22M, [H2O] = 0.10M, [CH3CO2H] = 0.010 M, [C2H5OH] = 0.010 M b. [CH3CO2C2H5] = 0.22 M, [H2O] = 0.0020 M, [CH3CO2H] = 0.0020 M, [C2H5OH] = 0.10 M c. [CH3CO2C2H5] = 0.88 M, [H2O] = 0.12 M, [CH3CO2H) = 0.044 M, [C2H5OH] = 6.0 M d. [CH3CO2C2H5] = 4.4 M, [H2O] = 4.4 M, [CH3CO2H] = 0.88 M, [C2H5OH] = 10.0 M e. What must the concentration of water be for a mixture with [CH3CO2C2H5] = 2.0M, [CH3CO2H] = 0.l0 M, and [C2H5OH] = 5.0 M to be at equilibrium? f. Why is water included in the equilibrium expression for this reaction?
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What does it mean to describe a reaction as reversible?
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