Question

Select the correct statement for a galvanic cell involving the following reaction:
$Zn\left(s\right)+C{u}^{2+}\left(aq\right)\rightleftharpoons Z{n}^{2+}\left(aq\right)+Cu\left(s\right)$

• A. Zinc rod act as sink for electrons
• B. The given redox process is spontaneous
• C. $C{u}^{2+}\left(aq\right)+2e^{-}\to Cu\left(s\right),$ takes place at anode
• D. $Zn\left(s\right)\to Z{n}^{2+}\left(aq\right)+2e^{-},$ takes place at cathode

Answer 1

The correct option is B The given redox process is spontaneous

Galvanic cell is also known as Voltaic cell. It converts the chemical energy liberated during the reaction to electrical energy. The chemical reaction will be a spontaneous reaction. In a electrochemical cell, the process of oxidation and reduction takes place simultaneously within the system. Thus, it is redox reaction.

The reactive metals have tendency to go into the solution phase, when in contact with their ions or their salt solution will act as anode.
The reactive metals when in contact with their aqueous solution, the ions in the solution have tendency to get deposited on the metal rod will act as cathode.
Thus, in the given cell reaction,
$Zn$ is getting oxidised and $Cu$ is getting reduced.
At anode :$Zn\left(s\right)\to Z{n}^{2+}\left(aq\right)+2e^{-}$
At cathode : $C{u}^{2+}\left(aq\right)+2e^{-}\to Cu\left(s\right)$

Thus, electron are generated in zinc rod. So, it act as source for electrons
Thus, statement (a), (c) and (d) are wrong.