Electrochemical Series

Chemistry ⇒ Redox Reactions and Electrochemistry

Electrochemical Series starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Electrochemical Series. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 12

Arrange the following metals in order of increasing reducing power based on their standard electrode potentials: Na, Fe, Cu.

Calculate the cell potential for a cell made of Fe²⁺/Fe (E° = -0.44 V) and Ag⁺/Ag (E° = +0.80 V).

Calculate the standard cell potential for the reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s). Given E°(Zn²⁺/Zn) = -0.76 V, E°(Cu²⁺/Cu) = +0.34 V.

Describe how the electrochemical series can be used to select suitable metals for sacrificial protection.

Describe the relationship between the position of a metal in the electrochemical series and its tendency to lose electrons.

Describe the trend in oxidizing power as you move down the electrochemical series.

Explain how the electrochemical series helps in predicting the products of electrolysis.

Explain why copper cannot displace zinc from zinc sulfate solution, using the electrochemical series.

Explain why gold does not corrode easily, based on its position in the electrochemical series.

Explain why lithium is placed above potassium in the electrochemical series, even though potassium is more reactive in water.

Explain why sodium cannot be obtained by the reduction of its salts using carbon, based on the electrochemical series.

If the standard electrode potential of Ag⁺/Ag is +0.80 V and that of Fe²⁺/Fe is -0.44 V, which is the stronger oxidizing agent?

The standard electrode potential of Zn²⁺/Zn is -0.76 V and that of Cu²⁺/Cu is +0.34 V. Which metal will displace the other from its salt solution?

What is the electrochemical series?

A galvanic cell is constructed using the following half-cells: Half-cell 1: MnO₄^- + 8H⁺ + 5e^- → Mn²⁺ + 4H₂O, E° = +1.51 V Half-cell 2: Fe³⁺ + e^- → Fe²⁺, E° = +0.77 V Calculate the standard cell potential and identify the substance that will be reduced.

A student claims that magnesium can reduce iron(III) ions to iron metal in aqueous solution. Use the electrochemical series to justify whether this claim is correct.

Consider the following half-reactions and their standard electrode potentials: Zn²⁺ + 2e^- → Zn(s), E° = -0.76 V Pb²⁺ + 2e^- → Pb(s), E° = -0.13 V Which metal will act as the anode in a galvanic cell constructed from these two half-cells?

Explain why potassium is a better reducing agent than calcium, based on their positions in the electrochemical series.

Explain, using the electrochemical series, why it is not possible to store a solution of silver nitrate in a copper vessel.

Given the following standard electrode potentials: E°(Al³⁺/Al) = -1.66 V, E°(Fe²⁺/Fe) = -0.44 V, E°(Cu²⁺/Cu) = +0.34 V. Predict whether iron will displace copper from a solution of copper(II) sulfate and justify your answer using the electrochemical series.