(C) In a $Daniel$ cell,the copper electrode acts as the cathode. \\ During the operation of the cell,cations in the electrolyte move toward the cathod

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Cations move toward copper electrode which is cathode.

(C) In a $Daniel$ cell,the copper electrode acts as the cathode. \\ During the operation of the cell,cations in the electrolyte move toward the cathode (copper electrode) to maintain electrical neutrality,where reduction takes place. \\ Therefore,statement $(c)$ is correct.

Class 12 Chemistry Electrochemistry Electrochemical cells

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Which of the following statements is true for the electrochemical $Daniel$ cell?

AIIMS 2004 All AIIMS

A
Electrons flow from copper electrode to zinc electrode.
B
Current flows from zinc electrode to copper electrode.
C
Cations move toward copper electrode which is cathode.
D
Cations move toward zinc electrode.

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$A$ hypothetical electrochemical cell is shown below $A | A^{+} (xM) || B^{+} (yM) | B$. If the cell potential is $+0.20 \ V$,the cell reaction is :-

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The correct statement/s about a Galvanic cell is/are:
$(a)$ Current flows from cathode to anode
$(b)$ Anode is the positive terminal
$(c)$ If $E_{cell} < 0$,then it is a spontaneous reaction
$(d)$ Cathode is the positive terminal

MediumKCET 2025

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Arrange the following metals in the order in which they displace each other from the solution of their salts: $Al$,$Cu$,$Fe$,$Mg$,and $Zn$.

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The reaction $1/2 H_{2(g)} + AgCl_{(s)} \to H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$ occurs in the galvanic cell:

MediumIIT 1985

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Why is an external $emf$ of more than $2.2 \ V$ required for the extraction of $Cl_2$ from brine?

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Which of the following statements is true for the electrochemical $Daniel$ cell?

Similar Questions

$A$ hypothetical electrochemical cell is shown below $A | A^{+} (xM) || B^{+} (yM) | B$. If the cell potential is $+0.20 \ V$,the cell reaction is :-

The correct statement/s about a Galvanic cell is/are:$(a)$ Current flows from cathode to anode$(b)$ Anode is the positive terminal$(c)$ If $E_{cell} < 0$,then it is a spontaneous reaction$(d)$ Cathode is the positive terminal

Arrange the following metals in the order in which they displace each other from the solution of their salts: $Al$,$Cu$,$Fe$,$Mg$,and $Zn$.

The reaction $1/2 H_{2(g)} + AgCl_{(s)} \to H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$ occurs in the galvanic cell:

Why is an external $emf$ of more than $2.2 \ V$ required for the extraction of $Cl_2$ from brine?

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The correct statement/s about a Galvanic cell is/are:
$(a)$ Current flows from cathode to anode
$(b)$ Anode is the positive terminal
$(c)$ If $E_{cell} < 0$,then it is a spontaneous reaction
$(d)$ Cathode is the positive terminal