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  • Consider the following figure and answer the following questions.Cell ‘A’ has Ecell = 2 V and cell ‘B’ has Ecen = 1.1 V which of the two cells ‘A’ or ‘B’ will act as an electrolytic cell. Which electrode reactions will occur in this cell?

Consider the following figure and answer the following questions.

(i) Cell ‘A’ has Ecell = 2 V and cell ‘B’ has Ecell = 1.1 V which of the two cells ‘A’ or ‘B’ will act as an electrolytic cell. Which electrode reactions will occur in this cell?
(ii) If cell ‘A’ has Ecell = 0.5 V and cell ‘B’ has Ecell = 1.1 V, what will be the reactions at anode and cathode?

Answers (1)

(i) As the potential of ‘B’ is lower than the potential of ‘A’, it will act as the electrolytic cell. The reactions at electrode ‘B’ are shown below:

Cathode : Zn^{2+}+2e^{-}\rightarrow Zn(s)

Anode: Cu (s)\rightarrow Cu^{2+}+2e^{-}

(ii) At higher potential, Cell ‘B’ acts as a galvanic cell and the reactions will be:

Anode :Zn(s)\rightarrow Zn^{2+}+2e^{-}

Cathode : Cu^{2+}+2e^{-}\rightarrow Cu(s)

An electrolytic cell is an electrochemical cell that utilizes an external source of electrical energy to force a chemical reaction that would otherwise not occur. The external energy source is a voltage applied between the cell's two electrodes; an anode and a cathode, which are immersed in an electrolyte solution.

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