Question

Why is anode in a galvanic cell considered to be –ve and cathode to be +ve electrode?

Answer 1

In a Galvanic cell the two electrodes are dipped in two different electrolytic solutions and connected by a salt bridge. In the anode oxidation reaction takes place and in cathode reduction reaction takes place.

Complete step by step answer:
The electrochemical cell is defined as the instrument which converts the chemical energy of the spontaneous redox reaction into electrical energy.
The Galvanic cell is defined as the electrochemical cell which uses chemical reaction to generate electricity.
In a Galvanic cell the electric work is due to the Gibbs free energy of the spontaneous redox reaction. The Galvanic cell consists of two halves and both the half is linked by a salt bridge. Each half cell consists of a metallic electrode dipped in the electrolytic solution. The two half-cells are connected by a voltmeter and a switch externally.
In a Galvanic cell, an oxidation reaction occurs in anode. The oxidation is the loss of electrons. In cathode reduction takes place. The reduction is defined as gain of electrons.
In Galvanic cell, the anode is negatively charged as it has negative potential with reference to the electrolytic solution and it is connected to the negative terminal of the battery and cathode is positively charged as it has positive potential with reference to the electrolytic solution and it is connected to the positive terminal of the battery.
Therefore, the correct option is C.

Note:
When the electrodes are dipped in the same electrolytic solution, then salt bridge is not required. In an electrolytic cell the anode is considered as positive and cathode is considered as negative.