Advertisements
Advertisements
Question
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.
Solution
(i) Copper will deposit at cathode.
(ii) Copper will dissolve at anode.
Explanation:
In the electrolysis process of \[\ce{CuSO4}\] the following reactions occur at the half cell which is as follows:
At the cathode, the reaction goes this way,
\[\ce{Cu^{2+} + 2e^{-} -> Cu(s)}\]
At the anode, the reaction goes this way,
\[\ce{Cu(s) -> Cu^{2+} + 2e^{-}}\]
Here copper will be deposited at the cathode and copper will dissolve at the anode.
APPEARS IN
RELATED QUESTIONS
Following reactions occur at cathode during the electrolysis of aqueous sodium chloride solution:
Na+(aq) + e− ⟶ Na (s) E0 = 2.71 V
H+(aq) + e− ⟶ `1/2` H2 (g) E0 = 0.00 V
On the basis of their standard reduction electrode potential (E0) values, which reaction is feasible at the cathode and why?
How much charge is required for the following reduction:
1 mol of \[\ce{Cu^{2+}}\] to \[\ce{Cu}\]?
How much charge is required for the following reduction:
1 mol of \[\ce{MnO^-_4}\] to \[\ce{Mn^{2+}}\]?
Three electrolytic cells A, B, C containing solutions of \[\ce{ZnSO4}\], \[\ce{AgNO3}\] and \[\ce{CuSO4}\], respectively, are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?
Explain Faraday’s second law of electrolysis
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 ____________.
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.
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?
Assertion (A): During electrolysis of aqueous copper sulphate solution using copper electrodes hydrogen gas is released at the cathode.
Reason (R): The electrode potential of Cu2+/Cu is greater than that of H+/H2.
Select the most appropriate answer from the options given below:
