Home
Class 12
CHEMISTRY
In the cell represented by Pb(s)|Pb^(...

In the cell represented by
`Pb(s)|Pb^(2+)(1 M)||Ag^(+)(1M)|Ag(s)` the reducing agent is

A

Pb

B

`Pb^(2+)`

C

Ag

D

`Ag^(+)`

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    TARGET PUBLICATION|Exercise EVALUATION TEST|19 Videos
  • ELECTROCHEMISTRY

    TARGET PUBLICATION|Exercise CRITICAL THINKING|76 Videos
  • D AND F-BLOCK ELEMENT

    TARGET PUBLICATION|Exercise EVALUATION TEST|15 Videos
  • GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF ELEMENTS

    TARGET PUBLICATION|Exercise Evaluation Thinking|15 Videos

Similar Questions

Explore conceptually related problems

For the cell Cu (s) | Cu ^(2+) (aq) (0.1 M) || Ag ^(+) (aq) (0.01 M) | Ag (s) the cell potential E _(1) = 0.3095 V For the cell Cu (s) | Cu ^(+2) (aq) (0.01 M) || Ag ^(+) (aq)( 0. 001 M) | Ag (s) the cell potential = _______ xx 10 ^(-2) V. (Round off the Nearest Integer). [Use : (2.303 RT)/(F) =0.059 ]

The value of reaction quotient Q for the cell Zn(s)|Zn^(2+)(0.01M)||Ag^(o+)(1.25M)|Ag(s) is

The Nernst equation: Consider the following galvanic cell Pb(s) | Pb^(2+)(aq.) || Ag^(2+)(aq.) | Ag(s) (a) What is the quantitative change in the cell voltage on increas-ing the ion concentrations in the anode compartment by a factor of 10 ? (b) What is the quantitative change in the cell voltage on increas-ing the ion concentration in the cathode compartment by a factor of 10 Strategy: The conventional notation of the cell tells us that lead is the anode while silve is the cathode. Therfore, the cell reaction is Pb(s) + 2Ag^(+)(aq.) rarr Pb^(2+)(aq.) + 2Ag(s) The cell potantial (at 25^(@)C ) is given by the Nernst equation, where n = 2 and Q = C_(Pb^(2+))//C_(Ag^(+)) : E_("cell") = E_("cell")^(@)-(0.0592 V)/(n) "logQ" E_("cell")^(@)-(0.0592 V)/(n) "logQ" C_(Pb^(2+))/C_(Ag^(+))^(2)

An alloy of Pb-Ag weighing 1.08g was dissolved in dilute HNO_(3) and the volume made to 100 mL.A ? Silver electrode was dipped in the solution and the emf of the cell dipped in the solution and the emf of the cell set-up as Pt(s),H_(2)(g)|H^(+)(1M)||Ag^(+)(aq.)|Ag(s) was 0.62 V . If E_("cell")^(@) is 0.80 V , what is the percentage of Ag in the alloy ? (At 25^(@)C, RT//F=0.06 )

TARGET PUBLICATION-ELECTROCHEMISTRY-COMPETITIVE THINKING
  1. When same quantity of electricity is passed for half an hour, the amou...

    Text Solution

    |

  2. Two electrolytic cells containing molten solutions of nickel chloride ...

    Text Solution

    |

  3. In the cell represented by Pb(s)|Pb^(2+)(1 M)||Ag^(+)(1M)|Ag(s) the...

    Text Solution

    |

  4. De-electronation process in Nernst theory means .

    Text Solution

    |

  5. The electrode where de-electronation takes place acts as .

    Text Solution

    |

  6. Standard electrode potential for Sn^(4+)//Sn^(2+) couple is 0.15 V and...

    Text Solution

    |

  7. Given below are half-cell reactions

    Text Solution

    |

  8. The cell reaction of a cell is Mg+Cu^(2+) to Mg^(2+)+Cu (Given E(...

    Text Solution

    |

  9. Standard reduction potential of Au^(3+)//Au and Sn^(4+)//Sn^(2+) elect...

    Text Solution

    |

  10. The e.m.f of galvanic cell , with oxidation potentials of Zn = +0.76 V...

    Text Solution

    |

  11. The E(cell)^(@) value for Pt, H(2)|H^(+)||Ag^(+)|Ag is . [E(Ag//Ag^(+)...

    Text Solution

    |

  12. In the cell Zn|Zn^(2+)(1M)||H^(+)(1M)|H(2(g))|Pt Zn electrode is repla...

    Text Solution

    |

  13. The e.m.f of the following cell, Zn |ZnSO(4) (1M)||H^(+)(1M)|H(2(g))...

    Text Solution

    |

  14. For the electrochemicl cell, M|M^(+)||X^(-)|X E((M^(+)//M))^(@) = 0.44...

    Text Solution

    |

  15. At temperature of 298 K , the e.m.f. of the following electrochemical ...

    Text Solution

    |

  16. In the electrochemical cell: Zn|ZnSO(4)(0.01 M)||CuSO(4)(1.0M)|Cu ...

    Text Solution

    |

  17. Standard electrode potentials are Fe^(2+)//Fe, E^(@) = -0.44 V Fe^...

    Text Solution

    |

  18. Nernst equation for Zn((aq))^(2+)+2e^(-) to Zn((s)) is E(Zn^(2+)//Zn) ...

    Text Solution

    |

  19. Given E(Cr^(3+)//Cr)^(@)=-0.72V, and E(Fe^(2+)//Fe)^(@)=-0.42V The...

    Text Solution

    |

  20. The cell , Zn | Zn^(2+) (1M) || Cu^(2+) (1M) Cu (E("cell")^@ = 1. 10 V...

    Text Solution

    |