Home
Class 12
CHEMISTRY
Four moles of electrons were transferred...

Four moles of electrons were transferred from anode to cathode in an experiment on electrolysis of water. The total volume of the two gases (dry and at STP) produced will be approximately (in litres)

A

22.4

B

44.8

C

67.2

D

89.4

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Topper's Solved these Questions

  • REVISION EXERCISE

    AAKASH SERIES|Exercise SURFACE CHEMISTRY|45 Videos

  • REVISION EXERCISE

    AAKASH SERIES|Exercise VA GROUP ELEMENTS|26 Videos

  • REVISION EXERCISE

    AAKASH SERIES|Exercise CHEMICAL KINETICS|39 Videos

  • REDOX REACTONS

    AAKASH SERIES|Exercise Questions For Descriptive Answers|27 Videos

  • SOLID STATE

    AAKASH SERIES|Exercise PRACTICE SHEET - 5|30 Videos

Similar Questions

Explore conceptually related problems

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolyte cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly proportionation to the amount of charge passed through it. The mass of substance liberated at electrode is calculate using the following realation : m=(itE)/(96500) Here, E represent the equivalent mass and 96500 C is called the faraday constant. Faraday (96500 C) is the charge of 1 mole electron i.e., 6.023 xx 10^(23) electrons, it is used to liberate on gram equivalent of the substance. Calculate the volume of gas liberated at the anode at STP during the electrolysis of a CuSO_4 solution by a current of 1 A passed for 16 minutes and 5 seconds.

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolyte cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly proportionation to the amount of charge passed through it. The mass of substance liberated at electrode is calculate using the following realation : m=(itE)/(96500) Here, E represent the equivalent mass and 96500 C is called the faraday constant. Faraday (96500 C) is the charge of 1 mole electron i.e., 6.023 xx 10^(23) electrons, it is used to liberate on gram equivalent of the substance. The platinum electrodes were immersed in a solution of cupric sulphate (CuSO_4) and electric current is passed through the solution. After sometimes, it was observed that the colour of copper sulphate disappeared with evolution of a gas at the electrode. The colourless solution contains.

Two rigid adiabatic vessels A and B which initially, contain two gases at different temperature are connected by pipe line with value of negligible volume. The vessel 'A' contain 2 moles Ne gas (C_(p.m) = (5)/(2)R) at 300K, vessel 'B' contain 3 moles of SO_(2) gas (C_(p.m) = 4R) at 400K. The volume of A & B vessel is 4 and 6 litre respectively. The final total pressure (in atm) when value is opened and 12 Kcal heat supplied through it to vessels. [Use: R= 2 cal/mol, K and R= 0.08L. atm/mol K as per desire]

AAKASH SERIES-REVISION EXERCISE -ELECTROCHEMISTRY
  1. On passing 3F electricity through three cells containing fused Na2CO3 ...

    Text Solution

    |

  2. For the electrolytic production of NaClO4 from NaClO3 according to t...

    Text Solution

    |

  3. The quantity of electricity in Faradays required to reduce 1.23 gm of ...

    Text Solution

    |

  4. When 3.86 amperes current are passed through an electrolyte for 50 min...

    Text Solution

    |

  5. When 965 amp current is passed through aqueous solution of salt X usin...

    Text Solution

    |

  6. What is the approximate quantity of electricity (in coulomb) required ...

    Text Solution

    |

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

    Text Solution

    |

  8. One Faraday of electricity is passed separately through one litre of o...

    Text Solution

    |

  9. The resistance of 0.5 N solution of an electrolyte in a conductivity c...

    Text Solution

    |

  10. 0.05M NaOH solution offered a resistance of 31.69Omega in a conducti...

    Text Solution

    |

  11. The resistance of 0.05M KCl solution at 25^@C is 100 ohm in a cell wh...

    Text Solution

    |

  12. Aluminium displaces hydrogen from acids, but copper does not. A galvan...

    Text Solution

    |

  13. When E(Ag^(+) | Ag)^@ = 0.80 volt and E(Zn^(2+)|Zn)^@ = 0.76 volt, wh...

    Text Solution

    |

  14. Deduce from the following E^@ values of half cells, what combination o...

    Text Solution

    |

  15. The half cell reaction for the corrosion are , 2H^(+) + (1)/(2) O2 + ...

    Text Solution

    |

  16. A cell constructed by coupling a standard copper electrode and a stand...

    Text Solution

    |

  17. E^@ values of Zn^(2+), Zn and Cu^(2+), Cu are respectively -0.76 V a...

    Text Solution

    |

  18. E^@ of Fe|Fe^(2+) is +0.44V , E^@ of Cu|Cu^(2+) is -0.32V. Then in the...

    Text Solution

    |

  19. The standard reduction potentials of Ag, Cu, Co and Zn are 0.799, 0.33...

    Text Solution

    |

  20. The standard reduction potentials of Zn^(2+)//Zn,Cu^(2+)//Cu and Ag^(+...

    Text Solution

    |