Using the standard reduction potentials., calculate the equilibrium constant for each of the fol-lowing reactions at 298 K:(a) Cu(s) + 2 Ag*(aq) → Cu² (aq) + 2 Ag(s)(b) 3 Ce**(aq) + Bi(s) + H2O(I) → 3 Ce* (aq) +BiO*(aq) + 2 H*(aq)(c) N,H3 (aq) + 4 Fe(CN) (aq) → Nz(8) +5H*(aq) + 4 Fe(CN),

Interpretation - To calculate the equilibrium constant using standard reduction potentials.

Answered: Using the standard reduction…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Using the standard reduction potentials , calculate the equilibrium constant for each of the fol- lowing reactions at 298 K: |(a) Fe(s) + Ni²*(aq) → Fe2*(aq) + Ni(s) (b) Co(s) + 2 H*(ag) → Co2* (aq) + H2(8) (c) 10 Br (ag) + 2 MnO, (aq) + 16 H*(aq) 2 Mn2+(aq) + 8 H,0(1) + 5 Br,(1)
Balance the following reaction in acidic solution. Fe?+ (ag) + MnO, (aq) → Fe+ (ag) + Mn²+(aq) Fill in the coefficients and substances for the balanced overall equation. Note: Do NOT leave any coeffient fields empty. If the coefficient is 1, choose "1" as opposed to leaving it blank. Fe2+ + MnO,¯ + 4 Fe3+ + Mn2+ +
Complete and balance this equation by the method of half-reaction.
Balance the following redox reaction in aqueous basic solution: 3- NO3 (ag) + Fe(CN),- → NO(9) + Fe(CN)6' + Fe(CN)6 (aq) (ад)
Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells. 2+ + (a) Fe(s) | Fe (aq) || Ag (aq) | Ag(s) V 2+ (b) Cd(s) | Cd²+ (aq) || Cr³+ (aq) | Cr(s) 2- 2+ (c) Cd(s), CdS(s) | S (aq) || Sn (aq) | Sn(s) V
7. Please answer the following questions. (a) Given the following reduction potentials Cd (OH)2 (s) + 2e → Cd (s) + 2 OH (aq) Eºred = -0.76 V NIO(OH) (s) + H₂O (1) + e → Ni(OH)2 (aq) + OH (aq) Eºred = +0.49 V Calculate the standard emf of the nickel-cadmium (nicad) rechargeable battery. *hint: the reaction for the discharge of nicad battery is: Cd (s) + 2 NIO(OH) (s) + 2 H₂O (1)→ 2Ni(OH)2 (aq) + Cd(OH)2 (s) (b) A typical nicad voltaic cell generates an emf of +1.30 V. Why is there a difference between this value and the one you calculated in part (b)? (c) Calculate the equilibrium constant for the overall nicad reaction based on this typical emf value.
Write balanced half-reactions for the following redox reaction: 3+ 2+ Cu* (aq) 2 Cr³+ (aq) +14 OH(aq) + 6 Cu²+ (aq) Cr₂O²(aq)+7H₂O()+6 reduction: oxidation:
Given the following half-reactions, 2 103 (aq) + 12H*(aq) + 10 e → 12(s) + 6H2O Fe2* (aq) → Fe3* (aq) + e" write the balanced overall reaction. 2103 - (aq) + 12 H* (aq) + Fe 2* (aq) → Fel2 (s) + 6 H2O o 2 103 (aq) + 10 Fe²* (aq) → l2 (s) + 10 Fe³+ (aq) 2 103 - (aq) + 12 H* (aq) + Fe 2* (aq) → 12 (s) + Fe3+ (aq) + 6 H20 2 103 - (aq) + 12 H* (aq) + 10 Fe 2* (aq) → 12 (s) + 10 Fe3+ (aq) + 6 H20
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: (aq) + 2Cu+ (aq) → Pb(s) + 2Cu²+ (aq) AG° Pb²+ = Pb²+ (aq) + 2e¯ → Pb(s) Ee = -0.126 V red 2+ Cu²+ (aq) + e → Cu+ (aq) Fº red kJ K for this reaction would be = = 0.153 V + than one.
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A medical technican is working with the four samples of radionuclides listed in the table below. Initially, each sample contains 6.00 umol of the radionuclide. First, order the samples by decreasing initial radioactivity. Then calculate how long it will take for the amount of radionudide in each sample to decrease to 1/4 of the initial amount.

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