Question

Which of the following statements is correct about the given Daniell cell?

• A. This cell converts the electrical energy liberated during the redox reaction to chemical energy
• B. This cell has an electrical potential greater than $1.1$ V when concentration of $Z{n}^{2+}$ and $C{u}^{2+}$ ions by unity($1$ mol $d{m}^{-3}$)
• C. In this cell, zinc is acting as anode and copper is acting as cathode
• D. Redox reaction occurring in this cell is $C{u}_{\left(s\right)}+Z{n}_{\left(aq\right)}^{2+}\to C{u}_{\left(aq\right)}^{2+}+Z{n}_{\left(s\right)}$

Answer 1

The correct option is C In this cell, zinc is acting as anode and copper is acting as cathode

A galvanic cell is an electrochemical cell that derives electrical energy from spontaneous redox reactions taking place within the cell. It generally consists of two different metals connected by a salt bridge or individual half-cells separated by a porous membrane. Daniel cell is a galvanic cell.

$Zn\left(s\right)+C{u}^{2+}\left(aq\right)\to Z{n}^{2+}+Cu\left(s\right)$

This reaction is a combination of two half reactions whose addition gives the overall cell reaction:

(i) $C{u}^{2+}+2e^{-}\to Cu\left(s\right)$ (reduction half reaction)

(ii) $Zn\left(s\right)\to Z{n}^{2+}+2e^{-}$ (oxidation half reaction)

The reduction half-reaction occurs on the copper electrode while the oxidation half-reaction occurs on the zinc electrode. These two portions of the cell are also called half-cells or redox couples. The copper electrode may be called the reduction half-cell and the zinc electrode, the oxidation half-cell. In Daniel, cell Zinc acts as an anode and copper act as a cathode.

Hence, the correct answer is option $\text{C}$.