Electrochemical Series
Chemistry ⇒ Redox Reactions and Electrochemistry
Electrochemical Series starts at 11 and continues till grade 12.
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See sample questions for grade 11
A cell is constructed with Mg and Cu electrodes. The standard electrode potentials are: Mg2+/Mg = -2.37 V, Cu2+/Cu = +0.34 V. Calculate the standard cell potential.
Arrange the following in order of decreasing oxidizing power: Cl2, F2, Br2.
Arrange the following metals in order of increasing standard electrode potential: Zn, Fe, Cu.
Describe how the electrochemical series can be used to select suitable materials for making electrochemical cells.
Describe how the electrochemical series helps in predicting the feasibility of a redox reaction.
Describe the relationship between standard electrode potential and the tendency of a species to gain electrons.
Explain why fluorine is the strongest oxidizing agent in 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 potassium is a stronger reducing agent than copper.
Explain why silver does not react with dilute hydrochloric acid, based on the electrochemical series.
If the standard electrode potential of Ag+/Ag is +0.80 V and that of Zn2+/Zn is -0.76 V, what is the standard cell potential for the cell: Zn | Zn2+ || Ag+ | Ag?
If the standard electrode potential of Fe2+/Fe is -0.44 V and that of Cu2+/Cu is +0.34 V, which metal will act as the anode in a galvanic cell?
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?
What is the significance of a negative standard electrode potential?
Which ion is more likely to be reduced: Fe3+ or Cu2+?
