A galvanic cell consists of one half-cell that contains Ag( s) and Ag (aq), and one half-cell that contains Pb( s) and Pb 2+( aq). What species areproduced at the electrodes under standard conditions?Ag (aq) + e-→ Ag(s) E° = +0.80 VPb 2+(aq) + 2 e→ Pb( s) E° = -0.13 VPb²+(aq) is formed at the cathode, and Cu(s) is formed at the anode.Ag(aq) is formed at the cathode and, Pb(s) is formed at the anode.Pb(s) is formed at the cathode, and Ag (ag) is formed at the anode.Ag(s) is formed at the cathode, and Pb2+(aq) is formed at the anode.

Two half cell reactions are given and asked that which species obtain at cathode and anode. In both half cell reactions, reduction potentials are given, half cell which have more reduction potential get reduced and other half cell which have less reduction potential or more oxidation potential get oxidised. Oxidation accur at anode and reduction occur at cathode. Here Ag have more reduction potential +. 80V,so it get reduced at cathode and become Ag(s) . And pb have less reduction potential - 0.13V, it will be oxidised at anode,and become pb+2(aq) in solution. . So correct option is D. That means Ag get reduced and become Ag(s) at cathode. And pb get oxidised and become pb+2 (aq).

Science

Chemistry

A galvanic cell consists of one half-cell that contains Ag( s) and Ag *(aq), and one half-cell that contains Pb( s) and Pb 2+( aq). What species are produced at the electrodes under standard conditions? Ag (aq) + e→ Ag( s) E = +0.80 V Pb 2+(aq) + 2 e Pb( s) E = -0.13 V O Pb2+(ag) is formed at the cathode, and Cu(s) is formed at the anode. O Ag(ag) is formed at the cathode and, Pb(s) is formed at the anode. Pb(s) is formed at the cathode, and Ag*(ag) is formed at the anode. Ag(s) is formed at the cathode, and Pb2+(aq) is formed at the anode.

A galvanic cell consists of one half-cell that contains Ag( s) and Ag (aq), and one half-cell that contains Pb( s) and Pb 2+( aq). What species are produced at the electrodes under standard conditions? Ag (aq) + e→ Ag( s) E = +0.80 V Pb 2+(aq) + 2 e Pb( s) E = -0.13 V O Pb2+(ag) is formed at the cathode, and Cu(s) is formed at the anode. O Ag(ag) is formed at the cathode and, Pb(s) is formed at the anode. Pb(s) is formed at the cathode, and Ag(ag) is formed at the anode. Ag(s) is formed at the cathode, and Pb2+(aq) is formed at the anode.

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

A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28 Write the balanced overall reaction that powers the cell. Calculate Ecell for the redox reaction. (round to 2 decimal places) What is [Ni²+] when Ecell when reaches 0.03V? (round to 2 sig figs) V What happens at equilibrium? What is Ecell at equilibrium? [Ni²+] at equilibrium: [Co2+] at equilibrium: (round to 2 decimal places) (round to 2 sig figs) (round to 2 sig figs) V M M M
3.2 calculate the standard cell potential of the following cell at 250 Sn(s)|Sn*(aq)||Cu*(aq)|Cu(s) 2+ 2+
In the given electrochemical cell, what is the cathode half-reaction? Zn(s) | Zn2+(aq) || Fe3+(aq), Fe2+(aq) | Pt(s)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential CrO2−4 (aq)+4H2O(l)+3e−→ CrOH3(s)+5OH−(aq) =E0red−0.13V Cl2(g)+2e−→ 2Cl−(aq) =E0red+1.359V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits. V
A chemist designs a galvanic cell from the following two half-reactions Ered = +0.96 V NO3(aq) + 4H+ (aq) + 3e¯ → NO(g) + 2H₂O (1) Ered +0.153 V Cu²+ (aq) + e¯ → Cut (aq) The standard cell potential for this galvanic cell is [Select] The standard free energy for this galvanic cell is AG [Select] The equilibrium constant (K) for this galvanic cell is [Select] = V.
A galvanic cell is powered by the following redox reaction: MnO (aq) + 8H(aq) + 5 Cu* (aq) (aq) + 4H₂O(1) + 5 Cu²+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. - Mn²+ ローロ X 00 3
With explanation Find the standard change in free energy and the equilibrium constant for the galvanic cell resulting from the cell notation provided below. P(s)|Cr2+(aq),Cr3+(aq)|| Pb2+(aq)|Pb(s)
A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28
Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag^+(aq)+e^-→Ag(s) What mass of silver plates onto the cathode when a current of 7.9 A flows through the cell for 73 min ?
3) Draw a picture of the galvanic cell represented by the line notation below and then write the reduction half-reactions for each electrode. Also identify the anode and cathode for each half cell. Pt (s) | Fe3+ (aq), Fe2+ (aq) || Cr2O72-(aq), Cr3+ (aq), HA (aq) | Pt (s)
The cell potential for a voltaic cell composed of zinc and copper is 1.0 V under standard conditions. Zn(s) + Cu2+(aq) => Cu(S) + Zn2+(aq) What is the cell potential when one of the following deviations from standard conditions are made? A) [Zn2+] = 0.25 M; [Cu2+] = 0.25 M B) [Zn2+] = 0.25 M; [Cu2+] = 0.50 M C) [Zn2+] = 0.75 M; [Cu2+] = 0.75 M D) [Zn2+] = 0.75 M; [Cu2+] = 0.25 M E) [Zn2+] = 0.25 M; [Cu2+] = 0.75 M
What is the overall cell reaction and the standard cell potential of a galvanic cell employing the following half-reactions ? NiO 2(s) +2H 2 O+2e^ -. ---> Ni(OH) 2(s) +2OH^- (aq) E ^ 0 = 0.49V Fe(OH) 2(s) +2e^ - ----> Fe (s) +2OH^- (aq) E ^ 0 = - 0.88 V