Determine Ecell for the reaction: 2 Al(aq) +3 Zn2*(aq) →2 Al3+(aq) + 3 Zn(s). The half reactionsare:Al3 (aq)+3 e Alls) E =-1.676 VZn2+(aq) +2 e Znls) E=-0.763 V-0.913 V-2.439 VO 0.913 V2.439 V01.063 V

Answered: Image /qna-images/answer/65e5f0ee-d1a4-45e6-a6a4-a04463910a03.jpg

Determine Ecell for the reaction: 2 Al(aq) +3 Zn2*(aq) → 2 Al3+(aq) + 3 Zn(s). The half reactions are: A3 laq) +3 e Alls) E =-1.676 V Zn2+(aq) +2 e Znls) E=-0.763 V 10.913 V 12.439 V O 0.913 V O 2.439 V -1.063 V

Determine Ecell for the reaction: 2 Al(aq) +3 Zn2*(aq) → 2 Al3+(aq) + 3 Zn(s). The half reactions are: A3 laq) +3 e Alls) E =-1.676 V Zn2+(aq) +2 e Znls) E=-0.763 V 10.913 V 12.439 V O 0.913 V O 2.439 V -1.063 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 data below, the E0cell = 0.30 V for the reaction: Cr(s) + 3Fe3+(aq) → 3Fe2+(aq) + Cr3+(aq). Half-reactions E0(V) Cr3+(aq) + 3e- → Cr(s) -0.74 Fe2+(aq) + 2e- → Fe (s) -0.440 Fe3+(aq) + e- → Fe2+(aq) +0.771 TRUE OR FALSE
Which species of the following half-reactions will reduce Pb +2(aq)?I2(s) + 2 e- → 2 I-(aq) E° = +0.535 V2 H+(aq) + 2 e- → H2(g) E° = 0Pb+2(aq) + 2 e- → Pb(s) E° = -0.125 VZn+2(aq) + 2 e- → Zn(s) E° = -0.763 V
Consider the following half-reactions: Half-reaction E° (V) Hg2+(aq) + 2e Cu2+ → Hg(1) 0.855V *(aq) + 2e¯ → Cu(s) 0.337V Fe2+(aq) + 2e" - Fe(s) -0.440v| (1) The strongest oxidizing agent is: enter for ula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Fe2+(aq) oxidize Hg(1) to Hg2+(aq)? (6) Which species can be oxidized by Cu2+(aq)? If none, leave box blank.
What is the Ecell for the spontaneous reaction resulting from the combination of half-reactions (1) and (3) below? (1) HgO(s) + H2O(1) + 2e + Hg(l) + 20H (aq) (2) Zn(OH)2(s) + 2e → (3) Ag20(s) + H20(1) + 2e (4) B(OH)3(aq) + 7H*(aq) + 8e E° = 0.098 V Zn(s) + 20H"(aq) E° = -1.250 V Ag(s) + 20H (aq) E° = 0.342 V BH4 (aq) + 3H20(1) E° = -0.481 V -0.244 V 0.244 V 0.440 V -0.440 V -0.122 V
Consider the following half-reactions: Half-reaction E° (V) Br21) + 2e → 2Br (aq) 1.080V Sn2 (aq) + 2e" Sn(s)-0.140V Cr*(aq) + 3e Cr(s) -0.740V The strongest oxidizing agent is: enter symbol The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will Cr(s) oxidize Br (aq) to Br2(1)? Which species can be oxidized by Sn"(aq)? If none enter none.
Write the overall reaction for the Redox reaction (below) when it occurs in a basic environment. H3ASO4 (aq) + Zn (s) → AsH3 (1) + Zn²+ (aq) Steps for writing half-cell reactions and overall Redox reactions: 1. Balance atoms other than H and O by changing their coefficients 2. Balance the O's and H's by adding OH and/or H₂O 3. Add electrons to balance the charge 4. Add the Oxidation and Reduction equations once the electrons in each cancel out 5. Cancel out (or reduce to the lowest possible numbers) any other species that are present on both sides of the reaction More Information H3ASO4 + AsH3 Zinc + Zinc ions
7>) True or False
Given the reduction half-reactions Fe3*(aq) + 3e- Fe(s) E° = -0.036 V Mg2*(aq) + 2e- Mg(s) E° = -2.37 V determine the correct information for this reaction. 2 Fe3+(aq) + 3 Mg(s) 2 Fe(s) + 3 Mg2+*(aq) O Ecell° = +0.085 V and the reaction is nonspontaneous as written O Ecell° = -2.41 V and the reaction is spontaneous as written O Ecello = +2.33 V and the reaction is spontaneous as written O Ecelo = +2.41 V and the reaction is nonspontaneous as written
4
Please answer letters D, E, F only in the attached pic
Consider the following half-reactions: Half-reaction E° (V) |Cl2(g) + 2e¯ → 2C1 (aq) 1.360V Co2+(aq) + 2e Mn2+(aq) + 2e → Co(s) -0.280V → Mn(s)-1.180V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will CI"(aq) reduce Mn2+(aq) to Mn(s)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Half-Reaction E° (V) 2H* (aq) + 2e¯ - H2 (9) 0.000 Ag* (aq) + e¯ → Ag (s) 0.7996 2H20 (I) + 2e¯ - H2 (g) + 20OH" (aq) -0.8277 AI3+ (aq) + 3e¯ → Al (s) -1.676 H2O2 (aq) + 2H* (aq) + 2e¯ → 2H20 (1I) 1.776 Au+ (aq) + e¯→ Au (s) 1.692 I2 (s) + 2e¯ → 21¯ (aq) 0.5355 Au3+ (aq) + 3e¯ → Au (s) 1.498 2103- (aq) + 12H* (aq) + 10e¯ → I2 (s) + 6H2O (1) Mg2+ (aq) + 2e - Mg (s) 1.195 Ba2+ (aq) + 2e¯ → Ba (s) -2.912 -2.372 Br2 (1) + 2e¯ → 2B1¯ (aq) 1.066 Mn2+ (aq) + 2e" → Mn (s) -1.185 Ca2+ (aq) + 2e¯ → Ca (s) -2.868 Mno2 (s) + 4H+ (aq) + 2e¯ → Mn2+ (aq) + 2H20 (1) 1.224 Cl2 (g) + 2e¯ → 2C1- (aq) 1.35827 Mno4- (aq) + 8H* (aq) + 5e¯ → Mn2+ (aq) + 4H2O (1) 1.507 Co2+ (aq) + 2e¯ → Co (s) -0.28 Mnog- (aq) + 2H20 (I) + 3e¯ → MnO2 (s) + 40H¯ (aq) 0.595 Co3+ (aq) + e¯ → Co2+ (aq) 1.92 HNO2 (aq) + H+ (aq) + e¯ → NO (g) + H2O (I) 0.983 Cr2+ (aq) + 2e¯ → Cr (s) -0.913 N2 (g) + 4H2O (1) + 4e¯ → 40H" (aq) + N2H4 (aq) -1.16 Cr3+ (aq) + 3e¯ → Cr (s) -0.744 NO3- (aq) + 4H* (aq) + 3e¯ → NO (g) + 2H2O (1) 0.957 Cr3+…