Practical No. 05: Determination of Electrode Potential of Iron
XIII. Interpretation of Results
Electrochemical cell with zinc and iron electrodes produced measurable EMF. Iron’s reduction potential was calculated as approximately -0.44 volts, matching the standard value. Zinc is placed above iron in electrochemical series, indicating greater electropositivity.
XIV. Conclusions and Recommendations
- Conclusion: Zinc is more electropositive than iron (-0.76 V vs -0.44 V). Therefore zinc acts as sacrificial anode protecting iron from corrosion.
- Recommendation: Use clean electrodes and fresh electrolyte solutions for accurate measurements.
XV. Practical Related Questions & Answers
Q1. Define De-electronation & Electronation.
- Answer: De-electronation is the process of removal of electrons from an atom or ion, i.e., oxidation (loss of electrons). Electronation is the process of addition of electrons to an atom or ion, i.e., reduction (gain of electrons). At anode, de-electronation occurs, and at cathode, electronation occurs in an electrochemical cell.
Q2. Write the factors influence the electrode potential of iron.
- Answer: Factors influencing electrode potential of iron include:
- (i) Nature of the metal and its ions.
- (ii) Concentration of metal ions in solution.
- (iii) Temperature of the solution.
- (iv) Pressure (for gaseous electrodes).
- (v) Nature of the electrolyte.
- (vi) Surface condition of the electrode.
Q3. Write the applications of the electrode potential of iron in industries or technologies.
- Answer: Applications include:
- (i) Designing corrosion protection systems like sacrificial anodes and cathodic protection.
- (ii) Electroplating and galvanization of iron surfaces.
- (iii) Manufacturing of batteries and electrochemical cells.
- (iv) Determining the feasibility of redox reactions.
- (v) Metallurgy and metal extraction processes.
- (vi) Sensor and analytical applications.
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