Calculate the value of Eºcell for the following reaction as written: HINT: Identify what is being oxidized and what is being reduced. 2F- + Ba²+ (aq) ---> F2 + Ba(s) Standard Reduction Potentials in Aqueous Solutions at 25 °C Oxidizing Agent F₂ H₂O₂ MnO₂ + AU³+ + Na+ Ca²+ Ba²+ K+ Lit + +++++ 2e™ 2H+ + 2e™ 8H+ + 5e 3e™ e™ 2e™ 2e™ e™ ↑↑↑↑↑↑ Reducing Agent 2F 2H₂O Mn²+ + 4H₂O Au Na Ca Ba K Li Reduction Potential (V) 2.87 1.78 1.51 1.50 -2.71 -2.87 -2.91 -2.93 -3.04

Calculate the value of Eºcell for the following reaction as written: HINT: Identify what is being oxidized and what is being reduced. 2F- + Ba²+ (aq) ---> F2 + Ba(s) Standard Reduction Potentials in Aqueous Solutions at 25 °C Oxidizing Agent F₂ H₂O₂ MnO₂ + AU³+ + Na+ Ca²+ Ba²+ K+ Lit + +++++ 2e™ 2H+ + 2e™ 8H+ + 5e 3e™ e™ 2e™ 2e™ e™ ↑↑↑↑↑↑ Reducing Agent 2F 2H₂O Mn²+ + 4H₂O Au Na Ca Ba K Li Reduction Potential (V) 2.87 1.78 1.51 1.50 -2.71 -2.87 -2.91 -2.93 -3.04

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

Consider the standard reduction potentials and redox couples used in a galvanic cell. Unbalanced Half-Reaction E°(V) MnO4 (aq) + 3e MnO2(s) (at basic pH) 0.59 Fe3+(aq) + e- Fe2*(aq) 0.77 What is the balanced reaction taking place in the cell (in basic solution)? 2 H20(1) + Mn04 (aq) + 3 Fe3+(aq) → 3 Fe2*(aq) + MnO2(s) + 4 OH- MnO2(s) + 4 OH¯ + 3 Fe3+(aq) 3 Fe2+(aq) + 2 H20(1) + MnO4¯(aq) MO 3 Fe2*(aq) + 2 H2O(1) + MnO4¯(aq) MnO2(s) + 4 OH¯ + 3 Fe3+(aq) M 3 Fe2+(aq) + MnO2(s) + 4 OH → 2 H20(1) + MnO4 (aq) + 3 Fe3+(aq)
Consider the following standard reduction potentials in acid solution: Co2+ + 2e– ----> Co (s) E° = –0.28 V MnO4– + 8H+ + 5e– ---> Mn2+ + 4H2O E° = +1.51 V The strongest reducing agent listed above is:
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
Use the standard reduction potentials given below to predict if a reaction will occur when Mg metal is put into a 1 M aqueous Cd²+ solution. Cd(s) Eº = -0.403 V red Eº → Mg(s) Fred = -2.370 V Cd2+ (aq) + 2e → 2+ Mg²+ (aq) + 2e 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.) +
Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4H+ Fe3+ + e-= Fe²+ E° = 0.771 V 0, + 2 H* + 2 e¯2 H,0 E° = 1.229 V E° = V K = Is the overall reaction spontaneous as written? AG° = spontaneous not spontaneous
Consider the following standard reduction potentials: F2(g) + 2 e - 2 F (aq) E° = +2.87 V Mg2*(aq) + 2 e - Mg(s) E° = -2.37 V Under standard conditions, O Mg(s) is a stronger oxidizing agent than F (aq), and Mg2*(aq) is a stronger reducing agent than F2(g), O F (aq) is a stronger oxidizing agent than Mg(s), and F2(g) is a stronger reducing agent than Mg2*(aq). O F2(g) is a stronger oxidizing agent than Mg-"(aq), and Mg(s) is a stronger reducing agent than F (aq). O Mg2*(aq) is a stronger oxidizing agent than F2(g), and F(aq) is a stronger reducing agent than Mg(s).
What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal place. 2 Cu(s) + 2 Ag+ (aq) ⇒ Cu²+ (aq) + 2 Ag (s) = Note: Reference the Standard reduction potentials at 25 °C table for additional information. K = = x10
Calculate the standard free‑energy change for this reaction at 25 °C. A list of standard reduction potentials can be found in this table. 2Au3+(aq)+3Ni(s)↽−−⇀2Au(s)+3Ni2+(aq) Δ?∘= kJ/mol
Standard Reduction Potentials (Volts) at 25 °C F2 (g) + 2 e- 2 F- (aq) 2.870 O2(g) + 4 H3O+(aq) + 4 e- 6 H2O(l) 1.229 2 H2O(l) + 2 e- H2(g) + 2 OH-(aq) -0.828 Fe2+ (aq) + 2 e- Fe (s) -0.440 A 0.122 M neutral aqueous FeF2 solution is electrolyzed under 1 atm pressure using platinum electrodes.(a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials.Half-reaction at anode: + + -> + + Half-reaction at cathode: + + -> + + (b) What is the expected decomposition potential? _______ V
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.
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
Which of the following reactions occurs at the anode of an electrochemical cell composed of Zn│Zn2+(aq) and Fe│Fe2+(aq) half-cells? Their reduction potentials are as follows: Zn2+ + 2e– --> Zn; Eo = -0.763 V Fe2+ + 2e– --> Fe; Eo = -0.447 V (A) Zn2+ + 2e– --> Cr; (B) Zn --> Zn2+ + 2e–; (C) Fe --> Fe2+ + 2e–; (D) Fe2+ + 2e– --> Fe;