Question

The EMF of the cell, \[ \text{Mg}^{2+}(0.01M) \parallel \text{Sn}^{2+}(0.1M) \parallel \text{Sn at 298K} \] is:

• A. 2.17 V
• B. 2.51 V
• C. 2.23 V
• D. 2.45 V

Hint:

The Nernst equation can be used to calculate the EMF of electrochemical cells under non-standard conditions.

Answer 1

The Correct Option is B

Step 1: Use the Nernst Equation.
The Nernst equation is used to calculate the EMF of a cell at non-standard conditions: \[ E = E^\circ - \frac{0.0591}{n} \log \left( \frac{[ \text{Red} ]}{[ \text{Ox} ]} \right) \]
Step 2: Conclusion.
The EMF of the cell is calculated to be 2.51 V.
Final Answer: \[ \boxed{2.51 \, V} \]