Home
Class 12
CHEMISTRY
How long (in hours) must a current of 5....

How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60g of calcium from molten `CaCl_(2)`?

A

27.2 hours

B

8.03 hours

C

11.02 hours

D

16.08 hours

Text Solution

Verified by Experts

The correct Answer is:
D
`1^(st)` law of Faradays
The reduction reaction: `Ca^(2+) + 2e^(-) rarr Ca`
`therefore Q= 1.5 xx 96500 xx 2= 289500C`
Coulombs = ampere `xx` seconds
Seconds = 289500/5= 57900 seconds `(57900s)/(3600s) = 16.08` hours
Promotional Banner

Topper's Solved these Questions

  • ELECTRO CHEMISTRY

    ACCURATE PUBLICATION|Exercise 1 Mark Each|22 Videos

  • ELECTRO CHEMISTRY

    ACCURATE PUBLICATION|Exercise 3 Marks each|15 Videos

  • D & F BLOCK ELEMENTS

    ACCURATE PUBLICATION|Exercise 2 OR 5 MARKS QUESTIONS|61 Videos

  • HALOALKANES AND HALOARENES

    ACCURATE PUBLICATION|Exercise TRUE AND FALSE (1 MARK)|10 Videos

Similar Questions

Explore conceptually related problems

How much electricity in terms of faraday is required to produce? 20.0 g of Ca from molten CaCl_2

How much electricity in terms of Faraday is required to produce :20.0 g of Ca from molten CaCl_2 ?

How many moles of electrons are required to Produce 10.0 g of Al from molten Al_2O_3 ?

How many grams of silver could be plated out on a serving tray by elelctolysis of a solution containing silver in +1 oxidation state for a period of 8.0 hours at a current of 8.46 amperes? What is the area of the tray if the thickness of the silver plating is 0.0025 cm? density of silver is 10.5 g/cm^3 .

How much electricity in terms of Faraday is required to produce : 40.0 g of Al from molten A1203?

How much electricity in terms of faraday is required to produce? 40.0 g of AI from molten Al_2O_3

A solution of Ni(NO3)_2 is electrolyzed between platinum electrodes using a current of 5.0 amperes for 20 minutes. What weight of Ni will be produced at cathode ? The atomic mass of Ni = 58.7 a.m.u ?

Three conductivity cells A, B and C containing solutions of zinc sulphate, silver nitrate and copper sulphate respectively are connected in series. A steady current of 1.5 amperes is passed through them until 1.45 g of silver is deposited at the cathode of cell B. How long did the current flow ? What mass of copper and what mass of zinc got deposited in their respective cells ? (Atomic mass : Zn = 65.4 u, Ag = 108 u, Cu = 63.5 u)

How many Faradays of electricity are required to deposit 10 g of calcium from molten calcium chloride using intert electrode?

A layer of chromium metal 0.25 mm thick is to be plated on an auto bumper with a total area of 032 m^2 from a solution cantaining CrO_4^(2-) ? What current flow is required for this electroplating if the bumper is to be plated in 60s ? The density of chromium metal is 7.20g/ cm^3

ACCURATE PUBLICATION-ELECTRO CHEMISTRY-Numbericals Practice
  1. How long (in hours) must a current of 5.0 amperes be maintained to ele...

    Text Solution

    |

  2. Give cell is {:([Ni|Ni^(2+) ||Cu^(2+)|Cu]),(" (0.01m) (0.1m)"):} ...

    Text Solution

    |

  3. A cell raction is n (s)| Sn((0.50M))^(2+)//H((0.020M))^(+)//H(2)(g). C...

    Text Solution

    |

  4. Calculate the maximum work that can be obtained from the Daniell cells...

    Text Solution

    |

  5. The resistance of a 0.5 M solution of an electrolyte in a conductivity...

    Text Solution

    |

  6. The resistance of a 0.5 M solution of an electrolyte enclosed between ...

    Text Solution

    |

  7. A solution of CuSO4 is electrolysed for 10 minutes with a current of 1...

    Text Solution

    |

  8. Can Chlorine gas be stored in Copper Cylinder ? Given E(Cu^(+)//Cu)^(@...

    Text Solution

    |

  9. State and explain Kohlrausch's law. How would you determine the molar ...

    Text Solution

    |

  10. Write Nernst equation and calculate the e.m.f. of the following cell a...

    Text Solution

    |

  11. Write Nernst equation and calculate e.m.f. of the cell at 298 k. Mg(...

    Text Solution

    |

  12. Write Nernst equation and calculate the e.m.f of the following cell at...

    Text Solution

    |

  13. Calculate the standard Gibbs energy for the cell : Zn(s)+Zn^(2+)(aq)...

    Text Solution

    |

  14. Calculate the standard Gibbs energy for the cell : Zn(s)|Zn^(2+)(aq)...

    Text Solution

    |

  15. Calculate the standard Gibbs energy for the cell : Zn(s)|Zn^(2+)(aq)...

    Text Solution

    |

  16. The lamda^(@) values of KNO(3) and LiNO(3) are 145.0 and 110.1 S cm^(2...

    Text Solution

    |

  17. Write Nernst equation and calculate the e.m.f of the following cell at...

    Text Solution

    |

  18. The lamda^(@) values of KCl and KNO(3) are 149.9 and 144.9 S cm^(2)mol...

    Text Solution

    |

  19. The lamda^(@) values of NaCl and NanO(3) are 126.5 and 121.6S" "cm^(2)...

    Text Solution

    |

  20. The calculate the e.mf. Of the following cell at 298: Fe|Fe^(2+)(0.1...

    Text Solution

    |

  21. Can we store copper sulphate solution in an iron vessel ?

    Text Solution

    |