ELECTROCHEMISTRY • STANDARD REDUCTION POTENTIALS AND CONCENTRATION DEPENDENCIES INTRODUCTION LABORATORY SIMULATION Lowest reduction potential Reactions 1 Ag* + e" - Ag Pb2* + 2e" - Pb 3 Zn?* + 2e - Zn Cu2* + 2e" - Cu 5 Ni2* + 2e" - Ni Highest reduction potential

ELECTROCHEMISTRY • STANDARD REDUCTION POTENTIALS AND CONCENTRATION DEPENDENCIES INTRODUCTION LABORATORY SIMULATION Lowest reduction potential Reactions 1 Ag* + e" - Ag Pb2* + 2e" - Pb 3 Zn?* + 2e - Zn Cu2* + 2e" - Cu 5 Ni2* + 2e" - Ni Highest reduction potential

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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The table below shows the standard reduction potential of some biochemical reactions. As per the table, the molecule that would most readily undergo reduction is a) H2O b) O2 c) NADH d) NAD+
[References] a. Will dichromate ions oxidize chloride ions to free chlorine in acidic solution? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E (V) Cr 0,2 + 14H+ +6e 2Cr* + 7H2O +1.33 Cl2+2e 2C1 +1.36 O yes Ono b. Will Fe+ oxidize'Sn+ to Sn**? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction € (V) Fe* +e+ Fe²* +0.77 Sn +2e Sn²* +0.15 O yes Ono
19. According to the following reduction potentials which sentence is INCORRECT? Sn2*(aq) + 2e -Sn(s) Fe2 (aq) + 2e Fe(s) Zn²* (aq) + 2e -Zn(s) E° = -0.14 V E° = -0.44 V E° = -0.76 V * O Zn is more easily oxidized than Fe. O Sn acts as the anode and Zn as the cathode in the galvanic process. O Fe is more easily oxidized than Sn. O Zn is the most powerful reducing reagent. Sn is the most powerful oxidizing reagent.
A 0.25 M sodium chloride solution was prepared from analytical grade NaCl. Brian immersed a silver (Ag) electrode into the solution prepared. Solve the following problems. a) Calculate the concentration of silver in this solution. Given Ksp of AgCl is 1.82 x 10-10. b) Calculate the electrode potential of silver electrode using reduction potential below. Ag+ + e- ↔ Ag(s) E° = 0.799 V AgCl(s) ↔ Ag(s) + Cl¯ E° = 0.222 V
Given the following reduction potentials, calculate the standard emf of the cell: Cd1OH221s2 + 2 e- ¡ Cd1s2 + 2 OH-1aq2 E° red = -0.76 V NiO1OH21s2 + H2O1l2 + e- ¡ Ni1OH221s2 + OH-1aq2 E° red = +0.49 V
cator=assignment-take [Review Topics] [References] Use the References to access important values if needed for this question. Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: I2 (s) + Co(s) → 21 (aq) + Co²+ (aq) Hìnt: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. K = than zero. AG° for this reaction would be romaining
[Review Topics] [References) Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: I2(s) + 2Cu*(aq)–→21(aq) + 2Cu²*(ag) Answer: kJ K for this reaction would be than one. Submit Answer Retry Entire Group 9 more group attempts remaining
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2Fe*(aq) + Ni(s)- →2FE?*(aq) + Ni²+(aq) 2+ Answer: kJ K for this reaction would be than one.
Use the References to access important values if needed for this question. Use the standard reduction potentials located in the "Tables' linked above to calculate the standard free energy change in kJ for the reaction: Zn*(aq) + 2Cu*(aq)Zn(s) + 2Cu²*(aq) Answer: kJ K for this reaction would be than one. Submit Answer Retry Entire Group 1 more group attempt remaining
Use the standard reduction potentials given below to predict if a reaction will occur when Cr metal is put into a 1 M aqueous 2+ Hg²+ solution. 2+ Hg²+ (aq) + 2e¯ → Hg(1) E red - = 0.855 V Cr³+ (aq) + 3e¯ → Cr(s) Ee -0.740 V red = If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) 2Cr(s) + 3Hg²+ (aq) 2Cr³(aq) + 3Hg(1)
# 3 change in kJ for the reaction: Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energ 2 Cr³+ (aq) + Cd(s) → 2Cr²+ (aq) + Cd²+ (aq) E Answer: Submit Answer K for this reaction would be F3 SA 4 R F F4 % [Review Topics] [References] Use the References to access important values if needed for this question. 5 T KJ Retry Entire Group G DII Cengage Learning Cengage Technical Support F5 A 6 Y than one. H 8 more group attempts remaining F6 & 7 U J E- F7 8 OO PrtScn | F8 K Home O F9 L 0 End F10 P Previous PgUp F11 [ 11 Next Save and Exit PgDn || 10:10 PM 12/2/2022 F12 1 14 Ins A Del Backspa 1
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.