Given the line notation, identify the anodic and cathodic reactions and overall reaction:
Ag(s)| AgCl(s) | Cl- (aq)|| Fe2+ (aq), Fe3+ (aq)|Pt(s)
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Given the line notation, identify the anodic and cathodic reactions and overall reaction: Ag(s)| AgCl(s) |...
QUESTION 8 Based on the following cell notation, write a balanced and complete redox reaction: Ca), sat. KCI Fe, Fe2 |Pt Ag) AgCl O A. Ag(s) +CI-(aq)Fe2+ AgCI (s) +Fe3+ = O B. AgCl (s)+ Fe2+ = Ag(s) +CI-(aq) Fe3+ CAg(s) +CI-(aq) + Fe2+ = AgCl(s) + Fe3+ D.Ag(s)CI-(aq) + Fe3+ AgCl(s)+ Fe2+ E. Ag(s)+CI-(aq)+2Fe2+= AgCI(s) +2FE3+
/ 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)
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),...
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. Anode half-reaction: РЫ Ag Pb(s) + 2 C1PCI () + 2e- Cathode half-reaction: AgCl(s) 2 AgCl(s) + 2e- Ag(s) + 2 C1- PbCI,() KCl(aq) KCl(aq) Shorthand notation: PbCl(s) Pb(s) Cl(aq) Cl(aq) Agcis) Ag(s) Answer Bank 2 AgCl(s) Pb(s) Cl(aq) AgCl(s) 2 Ag(s) PbCl () Ag(s) Incorrect
Attempt 2 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. Pb Anode half-reaction: Ag() +20 = A Ag(s) + 2e Cathode half-reaction: Agla + 2e Ag(s) + 2 CI PCL KC) AgCl) KCMag) Shorthand notation: Pb(s) PECI() Cr(4) Cl(aq) ACC) AC Answer Bank 2 AgCl) Cl(aq) Ag(s) 2 ARCO AgCl) PC1,() Pb(s)
Given the two reactions PbCl2(s)⇌Pb2+(aq)+2Cl−(aq), K3 = 1.87×10−10, and AgCl(s)⇌Ag+(aq)+Cl−(aq), K4 = 1.18×10−4, what is the equilibrium constant Kfinal for the following reaction? PbCl2(s)+2Ag+(aq)⇌2AgCl(s)+Pb2+(aq)
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...
Given the following reaction, balance it and write the line notation Ag+ + Cu(s) --> Ag(s) + Cu2+ HTML Editores
Exercise 19.49 Use line notation to represent the electrochemical cells for each of the following overall redox reactions. Part A 2Ag+ (aq) + Pb(s) +2Ag(s) + PbP (o) O Ag(s) Ag+ (aq)||Pb2+ (aq) Pb(6) O Ag+ (aq) Ag(0) Pb(s)[Pb (4) O Pb2+ (aq)|Pb()||Ag()|Ag (og) O Pb(s)|Pb2+ (aq)||Ag+ (aq)|A6(*) Submit Request Answer Part B 2010 (8) +21 (aq) +2010, (4) +10) O Pt()CIO; () CIO,()||()T()Ps) Pt(s) C10(e) C10, (w) (0) (0) Pt(s) O POT" (aq) (||C10(e)C10; ()Pt(s) OPt()LOT ()||CO, (w) CIO,()PC)...
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...