Solution:
2A) For the given reaction,
Sr(s) + Fe2+(aq) = Sr2+(aq) + Fe (s)
E°cell = E°(Fe2+/Fe) - E°(Sr2+/Sr)
E°cell = -0.44 V - (-2.90 V) = -0.44 V + 2.90 V
E° = + 2.46 V
E°cell is positive, hence reaction is spontaneous.
B) For the given reaction,
2Cr(s) + 3Cd2+ = 2Cr3+ + 3Cd
E•cell = E° Cd2+/Cd - E°Cr3+/Cr
= - 0.40 V - (-0.74 V)
= - 0.40 V + 0.74 V = + 0.34 V
Since, E°cell is positive, hence reaction is spontaneous.
2. Calculate the standard cell potential for each of the following redox reactions, and then predict...
tion 3 of 40 ) A voltaic cell employs the redox reaction: Zn (s) + Pb2+ (aq) — Zn2+ (aq) + Pb () where Pb2+ (aq) + 2e Zn2+(aq) + 2e Pb(s) E = -0.1262 V Zn(s) E = -0.7618 V The cell potential (Ecell) of this voltaic cell when [Pb2+1 = 1.10 M and [Zn2+) = 0.00110 Mis:
3) Calculate the standard cell potential E ^o and explaination for 4 please :) o Problem #3 Cont'd ... c. Zn (s)| Zn2+(aq, 1.0 M) || Fe2 (aq, 1.0 M) | Fe(s) d. Zn (s) | Zn2 (aq, 1.0 M) || Ag*(aq, 1.0 M) | Ag(s) tobeon 4. A student measured the standard cell potential of: 0 Jau 02 9isqsi Al(s) Al3 (aq) || Zn2 (aq) | Zn(s) There was a large percent error between the experimental E°cell and the...
For each set of materials below: i.Write the cell notation (line notation)for a galvanic cell and ii.Calculate the standard cell potential a. Pb(s), Zn(s), Pb2+(aq),Zn2+(aq) b. Ag(s), Fe(s), Ag+(aq),Fe2+(aq) c. Mg(s), Zn(s), Mg2+(aq),Zn2+(aq) d. Fe(s), Mg(s), Fe2+(aq), Mg2+(aq e. Ag(s), Pb(s), Pb2+(aq), Ag+(aq) 2. For each set of materials below: Write the cell notation (line notation) for a galvanic cell and Calculate the standard cell potential ii. a. Pb (). Zn (3), Pb2+(aq), Zn2+ (aq) 6. Ag (3), Fe (3),...
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s) + Cu?+ (aq) (aq) + Cu(s) B. Zn(s) + Cu(s) → Zn2+ (aq) + Cu2+ (aq) C. Zn2+ (aq) + Cu(s) Zn(s) + Cu2+ (aq) D. Zn (s) + 2 Cu(s) — Zn2+ (aq) + 2 Cu2+ (aq) (1pts) Identify the complete redox reaction for a Zn/Zn2+||Pb2+1Pb cell. A. Zn (s) + Pb(s) Zn2+ (aq) + Pb2+ (aq) B. Zn2+ (aq) + Pb(s) Zn(s)...
8. The standard cell potential (E°cell) for the reaction below is +1.10 V. Calculate the cell potential for this reaction when the concentration of [Cu2+] = 1.0 × 10-5 M and [Zn2+] = 3.5 M. Zn (s) + Cu2+ (aq) → Cu (s) + Zn2+ (aq)
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
Consider the following redox reactions. For each reaction, calculate the standard cell potential. See Table 12-2 from your book for a list of standard reduction potentials (or lecture notes CH12). A. Ag+ + Fe2+à Fe3+ + Ag(s) B. Zn2+ + Ni(s) à Ni2+ + Zn(s) C. 2Al3+ + 3Cu(s) à 2Al(s) + 3Cu2+
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table Ecell (measured) Reaction Quotient Q 1. Zn | Zn2(1.0M) || Cu2+(1.0 M) | Cu 2. Zn | Zn2+(1.0 M) || Cu2+(0.1 M) Cu 1.067 3. ZnZn2+(0.1 M) || Cu2+(1.0 M) | Cu 4. Zn | Zn2+(1.0 M) || Pb2+(1.0 M) | Pb 5. ZnZn2(1.0M) || Pb2+(0.1 M) | Pb 0.600 6. Zn | Zn2+(0.1 M) || Pb2+(1.0 M) I Pb 0.644 7. ZnZn2+(1.0 M)...
Many different ways have been proposed to make batteries. One cell is set up with copper and lead electrodes in contact with CuSO4(aq) and Pb(NO3)2 (aq), respectively. If the Pb2+ and Cu2+ concentrations are each 1.0 M, what is the overall cell potential? Pb2+ + 2e → Pb ER = -0.22 V ER = 0.34 V Cu2+ + 2e → Cu Choose 16. Choose best answer from drop-down menu: 2 points Given the following cell diagram, Al(s)AP+aq) || Cd2+(aq)| Cd...
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