Determine the Oxidizing and Reducing Agent in the reactions below: 3 Cl2(g) + 2 Fe(s) → 6 Cl– (aq) + 2 Fe3+(aq) Oxidizing Agent: Reducing Agent: Zn2+(aq) + NH4+(aq) → Zn(s) + NO3– (aq) Oxidizing Agent: Reducing Agent:

Using the reaction 2Al(s) + 3CuCl2·2H2O(aq) -> 3Cu(s) + 2AlCl3(aq) + 6H2O(l), determine the oxidation numbers and the oxidizating and reducing agents.

In the reaction FeCl 3 (s) + H2 (g) → 3HCI (g) + Fe (s), Cl acts as a reducing agent neither a reducing nor oxidizing agent

Assign oxidation states to all of the species in the following redox reaction. For the reactants, identify electron loss or gain, the species oxidized, the species reduced, the oxidizing agent and the reducing agent. Oxidation state Electron loss or gain Oxidized or reduced Reducing or oxidizing agent Mg(s) ♥ ◊ ŵ +2Fe³+ (aq)- → ◊ ♥ ◊ ◊ Mg2+ (aq) + 2Fe²+ (aq) ◊

Which of the following entities can act as both an oxidizing agent and as a reducing agent? Select one: O Cr²+ (aq) O Fe³+ (aq) O Cu²+ (aq) O Ag¹+ (aq) Which of the following is an entity that will reduce copper(II) ions and also oxidize metallic nickel? Select one: O Fe³+ (aq) O H₂O(1) O Sn²+ (aq) O Fe²+ (aq) Identify the SOA and the SRA A solution of iron (II) chloride is mixed with an acidified sodium nitrate solution. SOA SRA 5 425 4 45 ◆ Fe²+ (aq) Cl- (aq) H₂O (1) H+ (aq) Na+ (aq) ◆ NO3(aq) +H*(aq) 20 40

Identify the oxidizing agent in the reaction: 3 Mg(s) + 2NO3(aq) + 8 H*(aq) → 3 Mg2+ (aq) + 2NO(g) + 4H₂O NO3 (aq) Mg2+ (aq) H₂O NO(g) Mg(s) H+ (aq)

Identify the oxidizing agent and draw tie-lines to determine the reducing and oxidizing agents for the following reaction: 10 HNO3 (aq)  + I2 (s)  → 2 HIO3 (aq) + 10 NO2 (g)  +  4 H2O (l)

Formation of bromine from bromide. Assign oxidation numbers to each atom. Identify the oxidizing agent and the reducing agent. 2 Br-(aq) + Mn02(s) + 4 H1+(aq)→ Br2(s) + Mn²*(aq) + 2 H20(I)

Consider the following equation in aqueous solution: PO₃³⁻(aq) + SO₂(g) → PO₄³⁻(aq) + S²⁻(aq) The oxidation half-reaction is PO₃³⁻(aq) + H₂O(l) → PO₄³⁻(aq) + 2 H⁺(aq) + 2 e⁻ and the reduction half-reaction is SO₂ (g) + 4 H⁺(aq) + 6 e⁻ → S²⁻ (aq) + 2 H₂O(l). How many moles of electrons must be transferred in the overall reaction?

Identify the oxidizing and reducing agents in the following: 2MnO4−(aq) + 10 Cl−(aq) + 16 H+(aq) → 5 Cl2(g) + 2 Mn2+(aq) + 8 H2O(l)