Class 12 Exam  >  Class 12 Questions  >  A solution of Ni(NO3)2 is electrolysed b/w pl... Start Learning for Free
A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode?
Most Upvoted Answer
A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a...
W=zit ,z= E/F E = molar mass / n.f ,molar mass of nickel is 58 then w= 58 *0.5*20*60/2*96500 =144/965=0.149
Community Answer
A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a...
Electrolysis of Ni(NO3)2

Introduction:
Electrolysis is a process that uses an electric current to drive a non-spontaneous chemical reaction. It involves the breaking down of a compound into its constituent elements by passing an electric current through it. In this case, we will be electrolyzing a solution of Ni(NO3)2 using platinum electrodes to produce nickel at the cathode.

Given Information:
- Current (I) = 0.5 ampere
- Time (t) = 20 minutes = 20 x 60 seconds = 1200 seconds
- Ni(NO3)2 is the electrolyte

Step 1: Calculating the number of moles of electrons
To determine the amount of nickel produced, we need to find the number of moles of electrons transferred during the electrolysis. This can be calculated using Faraday's laws of electrolysis, which states that the amount of substance produced or consumed in an electrolysis reaction is directly proportional to the quantity of electricity passed through the cell.

The formula to calculate the number of moles of electrons (n) is:
n = (I x t) / (F x z)
Where:
- I is the current in amperes
- t is the time in seconds
- F is Faraday's constant (96485 C/mol)
- z is the number of electrons involved in the reaction

In this case, since Ni(NO3)2 is being electrolyzed, the balanced equation for the reaction at the cathode is:
Ni2+ + 2e- → Ni

From the balanced equation, we can see that 2 moles of electrons are involved in the reduction of 1 mole of Ni2+.

Therefore, z = 2 in this case.

Substituting the given values into the formula, we get:
n = (0.5 A x 1200 s) / (96485 C/mol x 2)

Step 2: Calculating the moles of Ni produced
Next, we need to calculate the moles of nickel produced at the cathode. Since each mole of nickel is produced by the transfer of 2 moles of electrons, the moles of nickel (nNi) can be calculated as:
nNi = n / 2

Step 3: Calculating the mass of Ni produced
Finally, we can calculate the mass of nickel produced by multiplying the moles of nickel by its molar mass (58.69 g/mol):
Mass of Ni = nNi x Molar mass of Ni

Conclusion:
By following the above calculations, we can determine the weight of nickel produced at the cathode during the electrolysis of Ni(NO3)2 using a current of 0.5 ampere for 20 minutes. The weight of nickel can be obtained by converting the moles of nickel produced to grams using its molar mass.
Explore Courses for Class 12 exam

Similar Class 12 Doubts

A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode?
Question Description
A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode?.
Solutions for A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode? in English & in Hindi are available as part of our courses for Class 12. Download more important topics, notes, lectures and mock test series for Class 12 Exam by signing up for free.
Here you can find the meaning of A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode? defined & explained in the simplest way possible. Besides giving the explanation of A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode?, a detailed solution for A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode? has been provided alongside types of A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode? theory, EduRev gives you an ample number of questions to practice A solution of Ni(NO3)2 is electrolysed b/w platinum electrodes using a current of 0.5 ampere for 20 minutes what weight of Ni will be produced at cathode? tests, examples and also practice Class 12 tests.
Explore Courses for Class 12 exam
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
10M+ students study on EduRev