Advertisements
Advertisements
Question
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.
Advertisements
Solution
(i) Copper will deposit at cathode.
(iii) Oxygen will be released at anode.
Explanation:
During electrolysis following reaction takes place at cathode:
\[\ce{Cu^{2+} + 2e^{-} -> Cu}\]
\[\ce{H^{-} + e^{-} -> 1/2 H_2}\]
Standard electrode potential of \[\ce{Cu^{2+}/Cu}\] is greater than \[\ce{H-/1/2 H2}\] therefore Cu will deposite at cathode.
APPEARS IN
RELATED QUESTIONS
Write any four applications of electrochemical series
Using the E° values of A and B, predict which is better for coating the surface of iron [E°(Fe+2/Fe) = -0.44V] to prevent corrosion and why?
Given: E° (A+2/A)=-2.37 V: E°(B+2/B)= -0.14V
Suggest a list of metals that are extracted electrolytically.
How much charge is required for the following reduction:
1 mol of Al3+ to Al?
How much charge is required for the following reduction?
1 mol of Cu2+ to Cu.
How much charge is required for the following reduction:
1 mol of \[\ce{MnO^-_4}\] to Mn2+?
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?
Write any two uses of H2SO4
What is the ratio of volumes of H2 and O2 liberated during electrolysis of acidified water?
(A) 1 : 2
(B) 2 : 1
(C) 1 : 8
(D) 8 : 1
State second law of electrolysis
Electrolytic cell uses electrical energy to bring about ____________.
According to Faraday’s First Law of Electrolysis, the amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the ____________.
In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?
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?
Time Required to deposite one millimole of aluminium metal by the passage of 9.65 ampere through aqueous solution of aluminium is
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).
On passing electricity through nitrobenzene solution, it is converted into azobenzene. The mass of azobenzene is ______ mg, if the same quantity of electricity produces oxygen just sufficient to burn 96 mg of fullerene (C60)·
