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.
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
On calculating the strength of current in amperes if a charge of 840C (coulomb) passes through an electrolyte in 7 minutes, it will be
- 1
- 2
- 3
- 4
Number of faradays of electricity required to liberate 12 g of hydrogen is:
Draw neat labelled diagram of electrolytic refining of blister copper
State second law of electrolysis
Explain Faraday’s second law of electrolysis
Write the name of the cell which is generally used in transistors. Write the reactions taking place at the anode and the cathode of this cell.
Electrolytic cell uses electrical energy to bring about ____________.
In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?
Given `1/a` = 0.5 CM–1, R = 50 ohm, N = 1.0 then equivalent conductance of electrolytic cell is
How much electricity in terms of Faraday is required to produce 40.0 g of \[\ce{Al}\] from molten \[\ce{Al2O3}\]?
(Given: Molar mass of Aluminium is 27 g mol−1.)
