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: Understanding the cell potential. The cell potential is calculated by subtracting the anode potential from the cathode potential. The two given standard electrode potentials are for the Sn^{4+}/Sn^{2+} couple (+0.15 V) and the Cr^{3+}/Cr couple (-0.74 V). 

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

Step 3: Conclusion. Thus, the cell potential is +0.89 V, corresponding to option (B). \vspace{10pt}