Based on the half-reactions and their respective standard reduction potentials below, which addition to an aqueous solution containing Fe3+ will result in a reduction of Fe3+ ? 02(g) + 4 H+ +4 e- → 2 H2O(1) 1.23 V Fe3+(aq) + e- Fe2+(aq) 0.77 V Cu2+(aq) + 2 e- → Cu(s) 0.34 V 2 H+(aq) + 2 e- → H2(g) 0.00 V Ni2+(aq) + + 2 e- → Ni(s) -0.26 V Fe2+(aq) + 2 e- → Fe(s) -0.45 V Water (H2O (I) ) O hydrogen gas oxygen gas aqueous copper(II) acetate O None

Based on the half-reactions and their respective standard reduction potentials below, which addition to an aqueous solution containing Fe3+ will result in a reduction of Fe3+ ? 02(g) + 4 H+ +4 e- → 2 H2O(1) 1.23 V Fe3+(aq) + e- Fe2+(aq) 0.77 V Cu2+(aq) + 2 e- → Cu(s) 0.34 V 2 H+(aq) + 2 e- → H2(g) 0.00 V Ni2+(aq) + + 2 e- → Ni(s) -0.26 V Fe2+(aq) + 2 e- → Fe(s) -0.45 V Water (H2O (I) ) O hydrogen gas oxygen gas aqueous copper(II) acetate O None

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

PLEASE HELP
Which of the following terms best describes the electrochemical reaction as written below.2 Pb 2+ ( aq) + 3 Au ( s) → 2 Pb ( s) + 3 Au 3+ ( aq)Standard Reduction PotentialsPb 2+ ( aq) + 2 e - → Pb ( s) -0.13 VAu 3+ ( aq) + 3 e - → Au ( s) 1.50 V The reaction is spontaneous. The reaction is not spontaneous. The spontaneity cannot be determined.
Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe*(aq) + B(s) + 6H,O(1) - Fe(s) + H,BO, (s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reductio Fe3+(aq) + 3 e¯ → Fe(s) E° = -0.04 V H,BO, (s) + 3 H,0*(aq) + 3 e- B(s) + 6 H,O(1) E° = -0.8698 V
Given the standard electrode reduction potentials, which reaction will occur spontaneously? Standard Reduction E° (V) Potentials Cu2+(aq) + e- → Cu+(aq) +0.15 V2+(aq) + 2e- V(s) -1.18 Mg2+(aq) + 2e- → Mg(s) -2.37 A) V2+ + 2Cu* → V + 2Cu2+ B) Mg2+ + V > V²* + Mg C) Mg2+ + 2Cu* → 2Cu2* + Mg D) Mg2+ + V2*→ Mg + V
Using the standard electrode potentials: Cl₂(g) +2e2Cl(aq) E° = +1.36 V; Cd2+ (aq) + 2e →→ Cd(s) E° = -0.40 V; Al³+ (aq) + 3e S Al(s) E° -1.66 V; Cu2+ (aq) + 2e → Cu(s) E° = +0.34 V. Decide which of the following reactions can happen spontaneously: Cd reduces Al³+ Cl₂ oxidizes Cd OCd2+ oxidizes Cu Cu2+ oxidizes CI
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Ch (g) + 2 e–→ 2 CI (aq) 1.360 02(g) + 4 H30*(aq) + 4 e→ 6 H20(1) 1.229 2 H20(1) + 2 e – H2(g) + 2 OH(aq) -0.828 |-0.403 Ca2* (aq) + 2 e" - → Cd (s) A 0.124 M neutral aqueous CdCl, 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: 6H,0 | 4H,0* + 4e Half-reaction at cathode: Cd2+ 2e Cd (b) What is the expected decomposition potential? 2.123 V +
Given the following standard reduction potentials, E°red, which species has the greatest tendency to be oxidized? S (s) + 2 H+ + 2e− → H2S (g) E°red = +0.144 V O2 (g) + 4 H+ + 4e− → 2 H2O (l) E°red = +1.229 V Sn2+ (aq) + 2e− → Sn (s) E°red = −0.137 V HERE ARE THE OPTIONS: O2 (g) S (s) Sn (s) H2S (g)
What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal place. Cu(s) + 2Ag+ (aq) ⇒ Cu²+ (aq) + 2 Ag (s) Note: Reference the Standard reduction potentials at 25 °C table for additional information. K = 0x10 X S
Calculate E°cell for the cell for the reaction 2 Ga(s) + 3 Sn4+(aq) → 3 Sn2+(aq) +2 Ga3+(aq).The standard reduction potentials are as follows: Ga3+(aq) + 3 e− → Ga(s) E° = –0.55 V Sn4+(aq) + 2 e− → Sn2+(aq) E° = 0.15V
What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal place. Cu(s) + 2Ag (aq) ⇒ Cu²+ (aq) + 2 Ag (s) Note: Reference the Standard reduction potentials at 25 °C table for additional information. K = x10 X S
Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe2+(aq) + 2 e– → Fe(s); E° = –0.41 V Pt2+(aq) + 2 e– → Pt(s); E° = 1.18 V Cr2O72–(aq) + 14 H+(aq) + 6 e– → 2 Cr3+(aq) + 7 H2O(); E° = 1.33 V Which of the following is the strongest oxidizing agent? Fe Pt Cr^3+ Fe^2+ Cr2O7^2-
Given the standard reduction potentials: Zn²+ (aq) + 2e-> Zn(s) Ag (aq) + e Ag(s) Which species is the best oxidizing agent? Zn(s) Ag(s) + Ag (aq) 2+ o Zn (aq) E =-0.76 V E = 0.80 V