Standard Electrode Potentials

Chemistry ⇒ Redox Reactions and Electrochemistry

Standard Electrode Potentials 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 Standard Electrode Potentials. 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

A cell is constructed with the following half-cells: Ag⁺/Ag (E° = +0.80 V) and Cu²⁺/Cu (E° = +0.34 V). Which electrode will act as the anode?

Arrange the following in order of increasing standard electrode potential: Fe²⁺/Fe (-0.44 V), Cu²⁺/Cu (+0.34 V), Zn²⁺/Zn (-0.76 V).

Calculate the standard 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 following cell: Mg(s) | Mg²⁺ (1 M) || Cu²⁺ (1 M) | Cu(s), given E°(Mg²⁺/Mg) = -2.37 V and E°(Cu²⁺/Cu) = +0.34 V.

Describe how the electrochemical series is constructed using standard electrode potentials.

Describe how the standard electrode potential of a half-cell changes if the concentration of ions is increased above 1 M.

Describe the conditions under which standard electrode potentials are measured.

Explain the significance of the electrochemical series in predicting the feasibility of redox reactions.

Explain why platinum is used as the electrode in the standard hydrogen electrode.

Explain why standard electrode potentials are intensive properties.

Explain why the standard electrode potential of a half-cell cannot be measured directly.

Explain why the standard electrode potential of fluorine (F₂/F^-) is the highest among all elements.

Given the following half-cell reactions and their standard electrode potentials: Fe³⁺ + e^- → Fe²⁺ (E° = +0.77 V), Fe²⁺ + 2e^- → Fe (E° = -0.44 V). Calculate the standard electrode potential for the reaction: Fe³⁺ + 3e^- → Fe.

If a metal has a standard electrode potential less than zero, what does this indicate about its reactivity compared to hydrogen?

If the standard electrode potential of a half-cell is more negative than that of the standard hydrogen electrode, will it act as an anode or cathode when connected to SHE?

If the standard electrode potential of Cu²⁺/Cu is +0.34 V and that of Zn²⁺/Zn is -0.76 V, what is the standard cell potential for the cell: Zn(s) | Zn²⁺ (1 M) || Cu²⁺ (1 M) | Cu(s)?

If the standard electrode potential of Pb²⁺/Pb is -0.13 V, will lead displace copper from a solution of CuSO₄?

State the Nernst equation for calculating electrode potential under non-standard conditions.

The standard electrode potential of Zn²⁺/Zn is -0.76 V. What does the negative sign indicate?

What is meant by the term 'standard electrode potential'?