
QUESTION 8 Based on the following cell notation, write a balanced and complete redox reaction: Ca),...
/ Question 8 / Write a balanced net ionic equation for the overall reaction represented by the cell notation below. Ag Agl|I || Fe2+, Fe3+ Pt Fe2+(ag) + Agi(s) — Fe3+(aq) + Ag(s) + F(ag) Fe?"(aq) + 21(aq) - Fe2+(aq) + 12(5) Fe3+(aq) + Ag(s) + 1-(aq) - Fe2+(aq) + AgI(s) Fe2+(aq) + Ag(s) +1-(aq) - Fe3+(aq) + AgI(s) Fe3+(ag) + Agi(s) - Fe2+(aq) + Ag(s) + (aq)
Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s) The reaction utilized by this cell is Question 8 options: Fe2+(aq) + 2Cl–(aq) --> Fe(s) + Cl2(g) Fe(s) + Cl2(g) --> Fe2+(aq) + 2Cl–(aq) 2Fe3+(aq) + 2Cl–(aq) --> 2Fe2+(aq) + Cl2(g) Fe3+(aq) + Cl–(aq) --> Fe2+(aq) + 1/2Cl2(g) 2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl–(aq)
II Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is the anode, and the one on the right is the cathode. 0 |Anode half-reaction: OD PbCl, (s) Pb(s) +201 – Cathode half-reaction: 2.AgCI() 2€ - PbCl,(s) KCl(aq) [ 285(0) AgCl(s) KCl(aq) 2 AgCl(s) Shorthand notation: Ag(s) | Pb(s) PbCl,(s) C1- (aq)] [c1-(aq)] | AgCl(s)) | 2 Ag(s) Answer Bank 2498) Ag(e) PbCly(@) Pb(8) 2.AgCI() CI+(ag) AgCl(s)
Question 5 (Q3) The cell notation for a voltaic cell with the following redox reaction is: Fe2+ (aq) + 2e → Fe(s) (oxidation) » Cr3+ (aq) + 3e" (reduction) Cr(s) Cr3+ (aq) | Cr (s) "Fe (s) | Fe2+ (aq) Cr3+ (aq) | Cr (s) " Fe2+ (aq) | Fe (s) Fe2+ (aq)| Fe (s) "Cr (s) [Cr3+ (aq) II Cr(s) | Cr3+ (aq) Fe2+ (aq)| Fe (s) None of the above
Choose the overall chemical reaction that takes place in a voltaic cell represented by the the following cell diagram Cr(s)| Cr3+(aq) || Fe3+(aq), Fe2+(aq) | Pt(s). Cr3+(aq) + 3Fe2+(aq) → Cr(s) + 3Fe3+(aq) O Cr(s) + 3Fe3+(aq) → Cr3+(aq) + 3Fe2+(aq) O Cr(s) + Fe2+(aq) → Cr3+(aq) + Fe3+(aq) Cr(s) + 3Fe2+(aq) → Cr3+(aq) + 3Fe3+(aq) O Cr(s) + 2Fe3+(aq) → Cr3+(aq) + 2Fe2+(aq)
1. Use the tabulated half-cell potentials to calculate AG for the following balanced redox reaction. SHow your work 2 Fe3+(aq) + 6 1(aq) 3 12(s)+ 2 Fe(s)
For each of the following galvanic cells (1) write out the conventional (overall) cell reaction and the two half reactions of which it is composed, (2) calculate the actual E for each cell a. Pt Br (aq) (0.75 M), Br2 (aq) (0.1 M)||Ci' (0.6 M) Cl2(Q) (0.2 atm), Pt b. Ag AgCl(), Cl- (0.5 M) || MinO4 (0.02 M), Mn2+ (0.15 M), H* (0.1 M) | Pt c. Cd Ca(NH3)42+ (0.04 M), NH3 (aq) (0.1 M) || Fe3+ (0.6 M),...
use the half reaction method to balance (SHOW ALL WORK) the following overall redox reaction describing the formation of acid mine drainage emanating from coal mines FeS2(s)+o2(g)+H2o(l)->FE(OH)3(s) +SO4 2-(aq) +H+(aq) balance redox entirely 1)FeS2+o2+h2o->fe2+ +So4 2- +h+ Balance redox entirely 2)2Fe2+ . + 1/2 O2 + 2H+ . ->2Fe3+ +H20 Balance this precipitation reaction Fe3+(aq) +3H2o(l) . -> F(OH)3 (s) +3H+(aq)
Question 14 (4 points) The standard cell notation for the following redox reaction is 2 Cr(s) + 3Fe2+ (aq) → 2 Cr3+ (aq) + 3Fe(s) Fe(s) Fe2+ (aq) | Cr3+ (aq) Cr(s) none of the choices 2 Cr(s) 2 Cr3+ (aq) || 3 Fe2+ (aq) 3 Fe(s) Cr(s) Cr3+ (aq) || Fe2+ (aq) | Fe(s) O3 Fe(s) 3 Fe2+ (aq) | 2 Cr3+ (aq) 2 Cr(s)
Choose the correct QUESTION 19 According to the following cell notation, the species that is undergoing oxidation is answer from the options below (a through e). Zn(s) Zn2+ (aq) || Mn2+(aq)|MnO2(3)| Pt() a. Mn2+ (aq) b. Zn2+ (aq) c. MnO2(3) d. Zn(s) e. Pt(s) Choose the correct answer from the In the following electrochemical cell, the cathode half reaction is options below (a through e). Mn(s) Mn2+ (aq) || Fe3+ (aq), F ), Fe2+ (aq)| Pt() 4. Fe3+(aq) + 6...