QUESTIONS and PROBLEMS 1. Write the equilibrium constant expression for ... Fe(H₂0)+(aq) + SCN (aq) = K₁ = [Fe NCS2+] [Fe³+] [SCN-1 Fe(H₂0) NCS²+ (aq) + H₂0(1) ૧૪૬૦ 19 2. Calculate an average value of the equilibrium constant from your experimental data. List the values of K, that you averaged; and include an error range with your value of K. (1.1 X102)-(9.3x10') -=935 = 3.5 x 10-3 3. In the equilibrium shown in Question 1, one bond is broken and another bond is formed. a) Consider the strength of the bond broken and the strength of the bond formed. What would the relative strengths of these bonds have to be for this particu- lar reaction to be exothermic? ... endothermic? b) Consider the relative numbers of Fe³+ ions, SCN ions and water molecules in any of your solutions. When Fe(H₂O), NCS²+ forms from the tons, this results (decrease/increase) in entropy. in a(n) c) Considering the entropy change of the forward direction (part b), is the for- ward reaction endothermic or exothermic? Justify. d) Therefore, which bond actually is stronger, the bond that is being made or the bond that is being broken? Justify.

QUESTIONS and PROBLEMS 1. Write the equilibrium constant expression for ... Fe(H₂0)+(aq) + SCN (aq) = K₁ = [Fe NCS2+] [Fe³+] [SCN-1 Fe(H₂0) NCS²+ (aq) + H₂0(1) ૧૪૬૦ 19 2. Calculate an average value of the equilibrium constant from your experimental data. List the values of K, that you averaged; and include an error range with your value of K. (1.1 X102)-(9.3x10') -=935 = 3.5 x 10-3 3. In the equilibrium shown in Question 1, one bond is broken and another bond is formed. a) Consider the strength of the bond broken and the strength of the bond formed. What would the relative strengths of these bonds have to be for this particu- lar reaction to be exothermic? ... endothermic? b) Consider the relative numbers of Fe³+ ions, SCN ions and water molecules in any of your solutions. When Fe(H₂O), NCS²+ forms from the tons, this results (decrease/increase) in entropy. in a(n) c) Considering the entropy change of the forward direction (part b), is the for- ward reaction endothermic or exothermic? Justify. d) Therefore, which bond actually is stronger, the bond that is being made or the bond that is being broken? Justify.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter27: Relative Stabilities Of Complex Ions And Precipitates Prepared From Solutions Of Copper(ii)

Section: Chapter Questions

Problem 1ASA

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This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of NH3(aq) to test tube #6: As a result of the colour change, what can be concluded about the [FeSCN2+(aq)]? Explain. Explain why the addition of NH3(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use chemical reaction in your explanation. Addition of heat/cold to test tube #7 & 8: As a result of the colour change, what can be concluded about the [FeSCN2+(aq)] when the temperature is increased? Explain. As a result of the colour…
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