Question

Arrange the following steps in the correct sequence to calculate the electrode potential of a polymer electrolyte system using the Nernst equation. \[ A.\ \text{Substitute value into the Nernst equation} \] \[ B.\ \text{Write the balanced electrode reaction} \] \[ C.\ \text{Identify the ionic species and their concentration in polymer electrolyte} \] \[ D.\ \text{Calculate the electrode potential under non-standard conditions} \] Choose the correct answer from the options given below:
• \( \mathrm{C \rightarrow B \rightarrow A \rightarrow D} \)
• \( \mathrm{B \rightarrow C \rightarrow A \rightarrow D} \)
• \( \mathrm{B \rightarrow A \rightarrow C \rightarrow D} \)
• \( \mathrm{A \rightarrow B \rightarrow C \rightarrow D} \)

• A. \( \mathrm{C \rightarrow B \rightarrow A \rightarrow D} \)
• B. \( \mathrm{B \rightarrow C \rightarrow A \rightarrow D} \)
• C. \( \mathrm{B \rightarrow A \rightarrow C \rightarrow D} \)
• D. \( \mathrm{A \rightarrow B \rightarrow C \rightarrow D} \)

Hint:

Always follow this sequence for Nernst equation problems:
• Write balanced reaction
• Identify ions and concentrations
• Substitute values
• Calculate electrode potential

Answer 1

The Correct Option is B

Concept: The Nernst equation is used to calculate electrode potential under non-standard conditions. The general Nernst equation is: :contentReference[oaicite:0]{index=0} where:
• \(E\) = electrode potential under non-standard conditions
• \(E^\circ\) = standard electrode potential
• \(n\) = number of electrons transferred
• \(Q\) = reaction quotient To apply the Nernst equation correctly, a systematic sequence of steps must be followed.

Step 1: Write the balanced electrode reaction first. Before using the Nernst equation, the electrode reaction must be known. This is essential because:
• The reaction determines electron transfer.
• The value of \(n\) depends upon the balanced equation.
• The reaction quotient \(Q\) depends on reactants and products. Thus, the first step is: \[ \boxed{ B.\ \text{Write the balanced electrode reaction} } \]

Step 2: Identify ionic species and concentrations. After writing the reaction, we identify:
• Ionic species involved
• Their concentrations
• Activities if necessary These quantities are needed for calculating the reaction quotient \(Q\). Thus, the next step becomes: \[ \boxed{ C.\ \text{Identify ionic species and their concentration} } \]

Step 3: Substitute values into the Nernst equation. Once:
• Balanced reaction is known
• Ionic concentrations are known we can substitute numerical values into the equation. Therefore, the next step is: \[ \boxed{ A.\ \text{Substitute values into the Nernst equation} } \]

Step 4: Calculate the electrode potential. After substitution and simplification, we finally compute: \[ E \] which is the electrode potential under non-standard conditions. Thus, the last step is: \[ \boxed{ D.\ \text{Calculate electrode potential} } \]

Step 5: Write the complete sequence. Combining all steps: \[ \boxed{ B \rightarrow C \rightarrow A \rightarrow D } \]

Step 6: Match with the options. This corresponds to: \[ \boxed{(2)} \] Additional Understanding: The Nernst equation connects electrochemistry with concentration changes. It explains:
• Concentration cells
• Battery voltage variations
• Electrochemical equilibrium Hence, identifying ionic concentrations correctly is extremely important. Final Conclusion: The correct sequence is: \[ \boxed{ B \rightarrow C \rightarrow A \rightarrow D } \] Hence, the correct answer is: \[ \boxed{(2)} \]