Home
Class 12
CHEMISTRY
A solution of Ni(NO(3))(2) is electrolys...

A solution of `Ni(NO_(3))_(2)` is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes what mass of Ni is deposited at the cathode?

Text Solution

Verified by Experts

Given current I = 5 A, `t = 20 xx60 s`, w= ?
`Q=Ixxt= 5xx20xx60 = 6000c`
Reaction for deposition Of Ni,
`Ni^(2+) + 2e^(-)`
`2 mol`
`2xx96500C` `rightarrow` Ni
1mol
` 58.7g`
Thus , `2xx96500 C` of electricity produces 58.7g Ni
`therefore 6000 C` of electricity would produce
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    VMC MODULES ENGLISH|Exercise Level- 0 (Short Answer Type - II ) (3Marks)|10 Videos

  • ELECTROCHEMISTRY

    VMC MODULES ENGLISH|Exercise Level-0 (Long Answer Type ) (5 Marks)|1 Videos

  • ELECTROCHEMISTRY

    VMC MODULES ENGLISH|Exercise Level-0 (Very short Answer Type )(1Marks)|1 Videos

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

    VMC MODULES ENGLISH|Exercise JEE ADVANCE (ARCHIVE)|30 Videos

  • ENVIRONMENTAL CHEMISTRY

    VMC MODULES ENGLISH|Exercise JEE Main (Archive)|39 Videos

Similar Questions

Explore conceptually related problems

A solution of Ni(NO_(3))_(2) is electrolyzed between platinum electrodes using a current of 5 amperes for 20 min. What mass of Ni is deposited at the cathode? (Atomic mass of Ni = 58.7) [Report your answer by rounding it upto nearset whole number]

A solution of Ni(NO_(3))_(2) is electrolyzed between platium electrodes using a current of 5A for 20 mi n . What mass of Ni is deposited at the cathode ?

A solution of Ni(NO_(3))_(2) is electrolysed between platinum electrodes using 0.1 Faraday electricity. How many mole of Ni will be deposited at the cathode?

A solution of CuSO_(4) is electroysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ? (Molar mass of Cu=63.5 g//mol)

A solution of CuSO_(4) is electroysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ? (Molar mass of Cu=63.5 g//mol)

A solution of copper (II) sulphate is electrolysed between copper electrodes by a current of 10.0 amperes passing for one hour. What changes occur at the electrodes and in the solution?

When an aqueous solution of AgNO_3 is electroysed between platinum electrodes, the substances liberted at anode and cathode are

108 g solution of AgNO_(3) is electrolysed using Pt electrodes by passing a charge of 0.1 F. The mass of resultant solution left is :

A well stirred solution of 0.1 M CuSO_(4) is electrolysed at 25^(@)C using platinum electrodes with current of 25mA for 6 hrs. If current efficiency is 50% At the end of the duration what would be the concentratin of copper ions in the solution ?

A dilute aqueous solution of Na_(2)SO_(4) is electrolyzed using platinum electrodes. The products at the anode and cathode are :