Home
Class 12
CHEMISTRY
An alloy of lead (Valency = 2) and thall...

An alloy of lead (Valency = 2) and thallium (valency = 1) containing 65% Pb and 35% Tl, by weight, can be electroplated onto a cathode from a solution. How many gram of this alloy will deposi in 9.65 hours using a constant current os 0.5 amp?
[Given that only these two elements deposit simultaneously in given mass ratio at cathode]
[Atomic weight Pb = 208, Tl = 200]

A

3.7 gm

B

22.5 gm

C

37.1 gm

D

24.9 gm

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTY

    GRB PUBLICATION|Exercise Conductance and Kohlrausch s law|40 Videos

  • ELECTROCHEMISTY

    GRB PUBLICATION|Exercise Reasoning type|28 Videos

  • ELECTROCHEMISTY

    GRB PUBLICATION|Exercise Thermodynamics in Electrochemistry|22 Videos

  • D-BLOCK ELEMENTS

    GRB PUBLICATION|Exercise Subjective Type|18 Videos

  • ENVIRONMENTAL CHEMISTRY

    GRB PUBLICATION|Exercise Straight objective type|40 Videos

Similar Questions

Explore conceptually related problems

One ampere of current is passed for 9650 seconds through molten AlCl_(3) What is the weight in grams of Al deposited at cathode? (Atomic weight of Al=27)

A solution of Ni (NO_(3))_(2) was electrolysed between platinum electrodes using current of 5 amp for 30 min . What is the mass of Ni deposited at the cathode ?

If the aqueous solutions of the following salts are electrolysed for 1 hour with 10 ampere current, which solution will deposit the maximum mass of the metal at cathode ? The atomic weights are : Fe=56, Zn=65, Ag=108, Hf=178 and W=184 .

What will be the current required to deposited on the cathode 39.4 g gold/hour from a solution containing a salt of gold (III)?

Lead storage battery has anode and cathode made up of Pb .

0.169 gram of copper is deposited on the cathode by a current of 32 milliamperes passing for 5 hours through a solution of copper sulphate. Determing the current efficiency. [ Atomic weight of Cu=63.6]

GRB PUBLICATION-ELECTROCHEMISTY-Faraday s Laws and Electrolysis
  1. Number of electrons lost dring electrolysis of 0.355g of Cl^(c-) is (N...

    Text Solution

    |

  2. Electrolysis of a solution of MnSO(4) in aqueous sulphuric acid is a m...

    Text Solution

    |

  3. An alloy of lead (Valency = 2) and thallium (valency = 1) containing 6...

    Text Solution

    |

  4. During the preparation of H(2)S(2)O(8) (per disulphuric acid) O(2) gas...

    Text Solution

    |

  5. A current of 9.95 amp following for 10 minutes, deposits 3 gm of a met...

    Text Solution

    |

  6. Four moles of electrons were transferred from anode to cathode in an e...

    Text Solution

    |

  7. Electrolytic reduction of 6.15 g of nitrobenzene using a current effic...

    Text Solution

    |

  8. A certain current liberates 0.5g of hydrogen in 2 hours. How many gra...

    Text Solution

    |

  9. All of the following affect the number of "mole"s of metal deposited d...

    Text Solution

    |

  10. What is the amount of chlorine evoled when 2 amperes of current is pas...

    Text Solution

    |

  11. A spoon to be electroplated with gold should be placed at:

    Text Solution

    |

  12. The two aqueous solutions, A (AgNO3) and B (LiCI), were electrolysed u...

    Text Solution

    |

  13. Time required to deposit one milli"mole" of aluminium metal by the pas...

    Text Solution

    |

  14. Which of the following statement is not correct about an inert electro...

    Text Solution

    |

  15. During the electrolysis of aqueous zinc nitrate.

    Text Solution

    |

  16. A currrent of 5.0 A flows for 4.0 h through an electrlytic cell contai...

    Text Solution

    |

  17. Which statement is not true about the electrolysis of a 1 M solution o...

    Text Solution

    |

  18. When water is electrolysed, hydrogen and oxygen gas are produced. If 1...

    Text Solution

    |

  19. How many "mole"s of electrons must be removed from each "mole" of toul...

    Text Solution

    |

  20. H(2)(g) is produced industrially by electrolysis of aq. NaCl using ine...

    Text Solution

    |