Advertisements
Advertisements
Question
A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?
Advertisements
Solution
Given: Current (I) = 5 A
Time (t) = 20 min = 20 × 60 = 1200 sec
Atomic weight of Ni = 58.70
The reaction takes place in the following manner:
\[\ce{Ni^{2+} + 2e- -> Ni}\]
Equivalent weight of Ni = \[\ce{\frac{Atomic weight}{Number of valence electrons}}\]
= \[\ce{\frac{58.70}{2}}\]
= 29.35
According to Faraday’s first law of electrolysis,
W = Z I t
= \[\ce{\frac{Equivalent weight}{96500} \times I \times t}\]
= \[\ce{\frac{29.35}{96500} \times 5 \times 1200}\]
= 1.825 g
APPEARS IN
RELATED QUESTIONS
96500 coulombs correspond to the charge on how many electrons?
Write any four applications of electrochemical series
Number of faradays of electricity required to liberate 12 g of hydrogen is:
If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?
How much charge is required for the following reduction?
1 mol of Al3+ to Al.
How many faradays of electricity are required to produce 13 gram of aluminium from aluminium chloride solution? (Given: Molar mass of Al = 27.0-gram mol–1)
Following reactions occur at cathode during the electrolysis of aqueous copper(II) chloride solution :
On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why ?
How much quantity of electricity in coulomb is required to deposit 1.346 × 10-3 kg of Ag in 3.5 minutes from AgNO3 solution?
( Given: Molar mass of Ag is 108 × 10-3 kg mol-1 )
Electrolytic cell uses electrical energy to bring about ____________.
What will happen during the electrolysis of aqueous solution of \[\ce{CuSO4}\] by using platinum electrodes?
(i) Copper will deposit at cathode.
(ii) Copper will deposit at anode.
(iii) Oxygen will be released at anode.
(iv) Copper will dissolve at anode.
What will happen during the electrolysis of aqueous solution of CuSO4 in the presence of Cu electrodes?
(i) Copper will deposit at cathode.
(ii) Copper will dissolve at anode.
(iii) Oxygen will be released at anode.
(iv) Copper will deposit at anode.
Assertion: Electrolysis of NaCl solution gives chlorine at anode instead of O2.
Reason: Formation of oxygen at anode requires overvoltage.
Consider the figure and answer the following question.
Cell ‘A’ has ECell = 2V and Cell ‘B’ has ECell = 1.1V which of the two cells ‘A’ or ‘B’ will act as an electrolytic cell. Which electrode reactions will occur in this cell?
When during electrolysis of a solution of AgNO3, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be ______.
Given `1/a` = 0.5 CM–1, R = 50 ohm, N = 1.0 then equivalent conductance of electrolytic cell is
On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode will be ______.
What is the quantity of electricity in Coulombs required to produce 4.8 g of Mg from molten MgCl2? How much Ca will be produced if the same amount of electricity was passed through molten CaCl2? (Atomic mass of Mg = 24 u, atomic mass of Ca = 40 u).
A current of 4 amp was passed for 2 hours through a solution of copper sulphate when 5.0 g of copper was deposited. The current efficiency is ______% (Cu = 63.5).
How much electricity in terms of Faraday is required to produce 40.0 g of Al from molten Al2O3?
(Given: Molar mass of Aluminium is 27 g mol−1.)
