Electrochemistry

Step 1: Understanding Reducing Power and Values
- The standard reduction potential ( ) of alkali metals determines their ability to lose electrons and act as reducing agents.
- A more negative value indicates a stronger reducing agent.
- The standard reduction potentials ( ) of alkali metals are: Step 2: Identifying the Weakest Reducing Agent
- The reducing power of alkali metals increases down the group due to decreasing ionization energy.
- Lithium ( ) has the most negative value, making it the strongest reducing agent.
- Sodium ( ) has the least negative value among the given options, meaning it is the weakest reducing agent.
Conclusion: Sodium (Na) is the weakest reducing agent as per its value.
Thus, the correct answer is Option (4): .

Step 1: Apply the Nernst Equation. Since , we set up the equation: Step 2: Solve for .

We can use Faraday’s law of electrolysis to calculate the atomic mass. The formula is: Where: - ,
- ,
- , - (since M is divalent). Rearranging the formula: Thus, the atomic mass of M is 63.47 u.

We are given V, J K , and K. We need to find . First, we find using the formula: where is the number of electrons transferred, which is 2 in this case. Now, we use the Gibbs
-Helmholtz equation: Rearranging for : Substituting the given values: