Question

Standard electrode potential for \( \text{Sn}^{4+}/\text{Sn}^{2+} \) couple is +0.15 V and that for the \( \text{Cr}^{3+}/\text{Cr} \) couple is -0.74 V. The two couples in their standard states are connected to make a cell. The cell potential will be:

To calculate the cell potential (\( E^\circ_{\text{cell}} \)), we use the standard electrode potentials of the given redox couples.

Given data:
\( E^\circ_{\text{Sn}^{4+}/\text{Sn}^{2+}} = +0.15V \)
\( E^\circ_{\text{Cr}^{3+}/\text{Cr}} = -0.74V \)

 

• A. +1.19 V
• B. +0.89 V
• C. +0.18 V
• D. +1.83 V
  \vspace{5pt}

Hint:

The cell potential is calculated by subtracting the anode potential from the cathode potential.

Answer 1

The Correct Option is B

Step 1: Cell Potential Determination. The cell potential is determined by subtracting the anode potential from the cathode potential. The provided standard electrode potentials are +0.15 V for the Sn^{4+}/Sn^{2+} couple and -0.74 V for the Cr^{3+}/Cr couple.

Step 2: Calculation. The cell potential is calculated as: \[ E_{\text{cell}} = E_{\text{cathode}} - E_{\text{anode}} = (+0.15 \, \text{V}) - (-0.74 \, \text{V}) = +0.89 \, \text{V} \]

Step 3: Result. The calculated cell potential is +0.89 V, which matches option (B). \vspace{10pt}