Solve for the cell potential E°cell in volts for the answer in item 1:Fe (s) + ½ O2 (g) + H2O → Fe2* (aq) + 20H'(aq)Use the following standard reduction potentials:Fe2* (ag) + 2e → Fe (s) E°red = -0.45 V2 02 (g)+ H20 + 2e→ 2 OH (ag) E°red = +0.40 VHint:Half Reactions:Ag* +e¯ → AgFe3+ +e¯ → Fe2+ E° = 0.77 VCalculation of Eeu (with positive value)Ag* +e¨ → AgFe2+ + Fe* +e"Cell Reaction: Ag* + Fe2+ → Fe³* + Ag_Egell = 0.03 VE° = 0.80 VE° = 0.80 V-E° = -0.77 V

Standard electrode potential is defined as the the potential of half reaction that is measured under…

Solve for the cell potential E°cell in volts for the answer in item 1: Fe (s) + ½ O2 (2) + H2O → Fe2* (aq) + 20H (aq) Use the following standard reduction potentials: Fe2+ (aq) + 2e → Fe (s) E°red = -0.45 V ½ 02 (g)+ H2O + 2e → 2 OH (aq) E°red = +0.40 V

Solve for the cell potential E°cell in volts for the answer in item 1: Fe (s) + ½ O2 (2) + H2O → Fe2* (aq) + 20H (aq) Use the following standard reduction potentials: Fe2+ (aq) + 2e → Fe (s) E°red = -0.45 V ½ 02 (g)+ H2O + 2e → 2 OH (aq) E°red = +0.40 V

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...

See similar textbooks

Similar questions

Given the standard electrode reduction potentials, which reaction will occur spontaneously?
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.
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Cr(OH)3 (s) +100H¯ (aq) +3Zn²+ (aq) → 2CrO²¯ (aq) +8H₂O (1) + 3 Zn (s) 0 x10 X
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG° for the following redox reaction. Round your answer to 3 significant digits. 6CI (aq)+2Cr0 (aq)+8H,0 (1) → 3Cl, (g)+2Cr(OH), (s) + 10OH (aq)
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Nit] = 0.00170 M and [Au] = 0.868 M. Standard reduction potentials can be found in this table. %3D 3 Ni(s) + 2 Au*(aq) 3 Ni?+(aq) + 2 Au(s) E = V
Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V
Consider the following standard reduction potentials: Zn2*(aq) + 2 e → Zn(s) E° = -0.76 V Mg2*(aq) + 2 e → Mg(s) E° = -2.37 V Ag*(aq) + e → Ag(s) E° = +0.80 V Which is the strongest oxidizing agent? Mg2*(aq) Zn2*(aq) Ag*(aq) 5:08 PM 90°F Partly sunny P Type here to search 8/6/2021
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. H₂(g) + 2OH(aq) + Zn²+ (aq) → 2H₂O (1) + Zn (s) kJ X S ? 1
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 3 significant digits. 2Cr(OH), (s)+100H (aq) +3C1₂(g) →2Cro (aq) +8H₂O()+6C (aq)