Rank the following species by increasing standard reduction potential: Au⁺(aq), F₂(g), ClO^–(aq).

Refer to the list of standard reduction potentials below:

Identify which of the following species can be reduced by Y.

Under standard conditions, list the following oxidizing agents in an acidic solution in order of increasing strength: Sn²⁺, MnO₄^–, N₂, Br₂, H₂SO₃. 

Br₂(l) + 2 e^– → 2 Br^–(aq)                                                    E°_red = +1.07 V
H₂SO₃(aq) + 4 H⁺(aq) + 4 e^– → S(s) + 3 H₂O(l)                 E°_red = +0.45 V
MnO₄^–(aq) + 8 H⁺(aq) + 5 e^– → Mn²⁺(aq) + 4 H₂O(l)        E°_red = +1.51 V
MnO₄^–(aq) + 2 H₂O(l) + 3 e^– → MnO₂(s) + 4 OH^–(aq)       E°_red = +0.59 V
N₂(g) + 5 H⁺(aq) + 4 e^– → N₂H₅⁺(aq)                                E°_red =  –0.23 V
N₂(g) + 4 H₂O(l) + 4 e^– → 4 OH^–(aq) + N₂H₄(aq)              E°_red = –1.16 V
Sn²⁺(aq) + 2 e^– → Sn(s)                                                     E°_red = –0.14 V

The following table lists a series of hypothetical reactions in aqueous solutions with their standard electrode potentials:

Identify the substance(s) that can oxidize Z²⁺.

Consider the following metal cations: 

Fe³⁺, Ni²⁺, Co²⁺, Ca²⁺

Identify which of the following is the best oxidizing agent.

Arrange the species in order of decreasing ability as a  reducing agent 

Sn⁴⁺, I₂, Ga³⁺ , Ca²⁺