**Question 13 of 20**Which of the following is the cell diagram for the reaction 3 Pb²⁺(aq) + 2 Al(s) → 3 Pb(s) + 2 Al³⁺(aq)?Options:A) Pb(s) | Pb²⁺(aq) || Al³⁺(aq) | Al(s)B) Pb²⁺(aq) | Pb(s) || Al³⁺(aq) | Al(s)C) Pb(s) | Pb²⁺(aq) || Al(s) | Al³⁺(aq)D) Al(s) | Al³⁺(aq) || Pb²⁺(aq) | Pb(s)E) Al³⁺(aq) | Al(s) || Pb(s) | Pb²⁺(aq)---**Explanation:**Each option represents a different possible cell diagram for an electrochemical cell involving lead and aluminum. In these diagrams, the single vertical line "|" indicates a phase boundary, and the double vertical line "||" represents the salt bridge or membrane separating the two half-cells. The substances on the left side correspond to the anode half-reaction, and those on the right to the cathode half-reaction.

In this question, correct cell diagram for the given reaction is to be determined. The given…

Which of the following is the cell diagram for the reaction 3 Pb²*+(aq) + 2 Al(s)→ 3 Pb(s) + 2 Als* (aq)? A) Pb(s) | Pb2*(aq) || Als*(aq) | Al(s) B) Pb²*(aq) | Pb(s) || Als*(aq) | Al(s) C) Pb(s) | Pb2*(aq) || Al(s) | AP*(aq) D) Al(s) | A*(aq) || Pb²*(aq) | Pb(s) E) AP*(aq) | Al(s) || Pb(s) | Pb²*(aq)

Which of the following is the cell diagram for the reaction 3 Pb²+(aq) + 2 Al(s)→ 3 Pb(s) + 2 Als (aq)? A) Pb(s) | Pb2(aq) || Als(aq) | Al(s) B) Pb²(aq) | Pb(s) || Als(aq) | Al(s) C) Pb(s) | Pb2(aq) || Al(s) | AP(aq) D) Al(s) | A(aq) || Pb²(aq) | Pb(s) E) AP(aq) | Al(s) || Pb(s) | Pb²(aq)

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

4. Write the overall net ionic equations for the following voltaic cells: (a) Zn(s)|Zn²"(aq)||Fe²*(aq)|Fe(s): (b) Zn(s)|Zn**(aq)||Fe**,Fe²*(aq)|C(s); (C = graphite is not involved in the reaction)
A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M
determine the cell notation for the redox reaction given below 3Cl2(g) + 2Fe(s) --> 6Cl-(aq) + 2Fe3+(aq) (see image)
999
3.2 calculate the standard cell potential of the following cell at 25C Sn(s)|Sn"(aq)||Cu?²*(aq)|Cu(s)
Q1
Calculate ΔG° for the redox reaction represented by the cell diagram Pt(s) | Cl2(g, 1 atm) || ZnCl2(aq, 1 M) | Zn(s).
What is the net reaction for the cell? Is it .44V or .22V?
Which of the following is the correct cell diagram for the reaction above at standard conditions. Select one: a. Zn (5)| Zn (aq) (1M) || (1M) Ag (aq) |Ag (s) b. Zn (s)| Zn (aq) (1M) || (1M) 2Ag (aq) 12A9 (s) c. Zn (s)| Ag (s) (1M) || (1M) Ag (aq) |Zn (aq) d. Ag (aq)| Zn (aq) (1M) || (1M) Zn (s)|Ag (s) e. 2 Zn (s)| Zn (aq) (1M) || (1M) Ag (aq) |2Ag (s) 2+ 2+
5.46/The potential of the cell Pt(s) | H₂(g) | HCl(aq)| AgCl(s) | Ag(s) is +0.312 V at 25°C. What is the pH of the electrolyte solution?
Give the standard line notation for each cell. (a) 2 IO3¯(aq) + 10 Cr²+ (aq) + 10 H+ (aq) ⇒ 10 Cr³+(aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Cr²+ (aq), IO3¯(aq), H+ (aq) || Cr³+ (aq), I2 (aq) | Pt(s) Pt(s) | Cr³+ (aq), I2 (aq) || Cr²+ (aq), 103¯(aq), H+ (aq) | Pt(s) Pt(s) | IO3¯(aq), H+ (aq), I2 (aq) || Cr²+ (aq), Cr³+ (aq) | Pt(s) Pt(s) | Cr²+ (aq), Cr³+ (aq) || IO3¯¯(aq), H† (aq), I₂ (aq) | Pt(s) (b) (c) (d) Co(s) + 2 Ag+ (aq) ⇒ Co²+ (aq) + 2 Ag(s) Co(s) | Ag+ (aq) || Co²+ (aq) | Ag(s) (aq) || Ag* (aq) | Co(s) Ag(s) | Co²+ 2+ Ag(s) | Ag+ (aq) || Co²+ (aq) | Co(s) 2+ Co(s) | Co²+ (aq) || Ag+ (aq) | Ag(s) H2O2(aq)+2 H*(aq)+2e O₂(g) + 2 H+(aq) + 2 e¯ → H2O2(aq) Pt(s) | H₂O₂ (aq) | 02 (9) || H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq) | Pt(s) Pt(s) | H₂O2 (aq), H+ (aq) || O2(g) | H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | O2(g) | H₂O2 (aq), H† (aq) || H₂O2 (aq), H† (aq) | Pt(s) 00 Mn²+ (aq) + 2 e → Mn(s) → 2H,O(l) 3+ Fe³+ (aq) + 3 e → Fe(s) Eº E° -1.18 V 3+ Fe(s) | Fe³+ (aq) || Mn²+ (aq) | Mn(s) Fe(s) | Mn²+ (aq)…
Consider this cell diagram for an electrochemical cell: Pt(s) | H2(g) | H*(aq) || Cu*(aq) | Cu(s) What is the overall balanced reaction for this redox reaction? O 2H (aq) + 2Cu(s) H2(g) + 2Cu (aq). O H2(g) + 2Cu'(aq) → 2H*(aq) + 2Cu(s) O H2(g) + 2Cu(s)H'(aq) + 2Cu'(aq) O H2(g) + Cu (aq) H'(aq) + Cu(s)