In the list of standard electrode potentials, the strongest oxidising agent is...

Which of the species strong oxidizing agent?

Cl₂(g) + 2e → 2Cl^-(aq) E^ocell = + 1.36 V

Cu²⁺(aq) + 2e → Cu(s) E^ocell = + 0.34 V

Ni²⁺(aq) + 2e → Ni(s) E^ocell = – 0.25 V

Ca²⁺(aq) + 2e → Ca(s) E^ocell = – 2.87 V

Arrange the species increasing order oxidizing agent?

Cl₂(g) + 2e → 2Cl^-(aq) E^ocell = + 1.36 V

Cu²⁺(aq) + 2e → Cu(s) E^ocell = + 0.34 V

Ni²⁺(aq) + 2e → Ni(s) E^ocell = – 0.25 V

Ca²⁺(aq) + 2e → Ca(s) E^ocell = – 2.87 V

A galvanic cell was set up using the Cu²⁺/Cu and Fe³⁺/Fe half-cells. The standard redox potentials for these half-cells are: Cu²⁺(aq)  +  2e^- →   Cu(s); E⁰ = +0.34 V

Fe³⁺(aq)  +  e^- → Fe²⁺(aq); E⁰ = +0.77 V

The oxidant and reductant reacting in this galvanic cell are, respectively:   

Consider the galvanic cell reaction Zn (s) + Cu²⁺ (aq) → Cu (s) + Zn²⁺ (aq) When the cell is running spontaneously, which is the only true statement?

If an electrochemical reaction is spontaneous, what will E^o_cell be?

If the standard cell potential, E^o_cell is negative, the reaction is?

Predict whether the following reaction occur spontaneously:

2Ag(s) + Br₂(g) ----------> 2Ag⁺(aq) + 2Br^-(aq)

Eº_Ag+/Ag = + 0.80 V Eº _Br2/_Br-= + 1.07 V