Home
Class 12
CHEMISTRY
Consider the reaction , PbO2 to PbO , De...

Consider the reaction , `PbO_2 to PbO , DeltaG_(298) lt 0 l SnO_2 to SnO , DeltaG_(298) gt 0` the most probable oxidation state of Pb and Sn will be

A

`Ph^(+4) , Sn^(+2) `

B

`Pb^(+4) , Sn^(+4)`

C

`Pb^(+2), Sn^(+3) `

D

`Pb^(+2) , Sn^(+4)`

Text Solution

Verified by Experts

The correct Answer is:
D
`PbO_2 to PbO , SnO_2 to SnO`
` underset(Pb^(+2))(DeltaG_(298) lt 0)" " underset(Sn^(+4))(DeltaG_(298) gt 0`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise PRACTICE SHEET -3 (LINKED COMPREHENSION TYPE QUESTIONS(PASSAGE-I))|3 Videos

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise PRACTICE SHEET -3 (LINKED COMPREHENSION TYPE QUESTIONS(PASSAGE-II))|3 Videos

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise PRACTICE SHEET -2 (MATCH THE FOLLOWING QUESTION )|8 Videos

  • DILUTE SOLUTIONS

    AAKASH SERIES|Exercise EXERCISE - 1.2|55 Videos

  • ELEMENTS OF D - BLOCK

    AAKASH SERIES|Exercise EXERCISE - 5.2|33 Videos

Similar Questions

Explore conceptually related problems

In the reaction, NO_(2)^(-)+OC l to NO_(3)^(-)+Cl^(-) , the oxidation state of chlorine

The E^(@) values for the changes given below are measured against NHE at 27^(@) C Cu^(2+) + e to Cu^(+) , E^(@) = + 0.15 V , Cu^(+) + e to Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e to Zn , E^(@) = - 0.76 V . The temperature coefficient of emf a cell designed as Zn|Zn^(2+) || Cu^(2+) || Cu is - 1.4 xx 10^(-4)v per degree . For a cell reaction in equilibrium DeltaG= 0 and DeltaG^(@) = -2.303 RT log K_(c) . The heat of reaction and entropy changes during the reaction are related by DeltaG = DeltaH - TDeltaS . The equilibrium constant constant for the reaction : Zn + Cu^(2+) iff Zn^(2+) + Cu is

The E^(@) values for the changes given below are measured against NHE at 27^(@) C Cu^(2+) + e to Cu^(+) , E^(@) = + 0.15 V , Cu^(+) + e to Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e to Zn , E^(@) = - 0.76 V . The temperature coefficient of emf a cell designed as Zn|Zn^(2+) || Cu^(2+) || Cu is - 1.4 xx 10^(-4)v per degree . For a cell reaction in equilibrium DeltaG= 0 and DeltaG^(@) = -2.303 RT log K_(c) . The heat of reaction and entropy changes during the reaction are related by DeltaG = DeltaH - TDeltaS . The E^@ for the reaction 2Cu^(+) to Cu^(2+) + Cu is :

The E^(@) values for the changes given below are measured against NHE at 27^(@) C Cu^(2+) + e to Cu^(+) , E^(@) = + 0.15 V , Cu^(+) + e to Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e to Zn , E^(@) = - 0.76 V . The temperature coefficient of emf a cell designed as Zn|Zn^(2+) || Cu^(2+) || Cu is - 1.4 xx 10^(-4)v per degree . For a cell reaction in equilibrium DeltaG= 0 and DeltaG^(@) = -2.303 RT log K_(c) . The heat of reaction and entropy changes during the reaction are related by DeltaG = DeltaH - TDeltaS . The decrease in free energy during the cell reaction in Zn | Zn^(2+) (1M)||Cu^(2+)(1M)|Cu , when its changes to 1M(Zn^(+2)) and 0.1M(Cu^(+2)) is .........

Pure H_(2)O_(2) is not very stable and decomposes in the presence of light or on standing or heating overset((-1))(H_(2)O_(2l))+overset((2-)) (H_(2)O_((l)))+overset((0))(O_(2(g))) The oxidation state of oxygen in H_(2)O_(2) is 1 it is oxidistion state of zero in O_(2) and is reduced to an oxidation state of -2 in H_(2)O . Thus, this decomposition is an example of auto oxidation reduction reaction or disproportionation reaction. Pure H_(2)O is

Pure H_(2)O_(2) is not very stable and decomposes in the presence of light or on standing or heating overset((-1))(H_(2)O_(2l))+overset((2-)) (H_(2)O_((l)))+overset((0))(O_(2(g))) The oxidation state of oxygen in H_(2)O_(2) is 1 it is oxidistion state of zero in O_(2) and is reduced to an oxidation state of -2 in H_(2)O . Thus, this decomposition is an example of auto oxidation reduction reaction or disproportionation reaction. 30-volume, hydrogen peroxide means

Consider the DeltaG_(f)^(0) and Delta H_(f)^(0) (kJ/mol) for the following oxides. Which oxide can be most easily decomposed to form the metal and oxygen gas?

AAKASH SERIES-ELECTROCHEMISTRY -PRACTICE SHEET -3 (SINGLE OF MORE THAN ONE OPTION QUESTIONS )
  1. The hydrogen electrode when placed in a buffer solution of CH3COONa an...

    Text Solution

    |

  2. For the cell Zn(s) | Zn^(2+) || Cu^(2+) | Cu(s) , the standard cell v...

    Text Solution

    |

  3. What is the reaction quotient , Q for the cell Ni((s)) | Ni^(2+) (0.19...

    Text Solution

    |

  4. A 1.0 M solution of Cd^(+2) is added to excess iron and the system is ...

    Text Solution

    |

  5. Standard electrode potential (E^(0)) for OCl^(-) // Cl^(-) and Cl^(-)/...

    Text Solution

    |

  6. The standard reduction potential of Cu^(2+) // Cu and Cu^(+) // Cu a...

    Text Solution

    |

  7. The oxidation potential of hydrogen half-cell will be negative if :

    Text Solution

    |

  8. Consider the cell Ag | AgBr | KBr || KCl | AgCl | Ag with EMF 0.059 V ...

    Text Solution

    |

  9. For the cell (at 298 K ) Ag((g)) // AgCl((s)) // Cl((aq))^(-) ||AgNO(3...

    Text Solution

    |

  10. The standard electrode potential of a metal-metal ion (Ag//Ag^(+)) and...

    Text Solution

    |

  11. underset((1atm25^@C))(Pt:H2)//underset((0.01M))(HCOOK)//// underset((0...

    Text Solution

    |

  12. For a Ag -Zn button cell , net reaction is : Zn((s) + Ag2 O((s)) to Zn...

    Text Solution

    |

  13. Consider the reaction , PbO2 to PbO , DeltaG(298) lt 0 l SnO2 to SnO ,...

    Text Solution

    |

  14. E("red")^(0) (Standard reduction potential ) of different half-cells a...

    Text Solution

    |

  15. For a reaction in a galvanic cell the value of -DeltaG^(@) at certain ...

    Text Solution

    |

  16. Which of the following statement are correct regarding to galvanic cel...

    Text Solution

    |