Question

which statement about the reaction is true? fe + 3o₂ → 2fe₂o₃ oxygen has an oxidation state of -2 in fe₂o₃. o₂ is the reducing agent. fe is the oxidizing agent. fe has an oxidation state of zero in fe₂o₃

Explanation:

Step1: Determine oxidation state of oxygen in \(Fe_2O_3\)

Let oxidation state of \(Fe\) be \(x\) and of \(O\) be \(y\). In \(Fe_2O_3\), using the rule that sum of oxidation states in a neutral compound is zero: \(2x + 3y=0\). Oxygen (in oxides, except peroxides and super - oxides) has an oxidation state of \(y = - 2\). Substituting \(y=-2\) gives \(2x+3\times(-2) = 0\), \(2x=6\), \(x = + 3\).

Step2: Analyze oxidizing and reducing agents

• Oxidizing agent: Substance that gains electrons (is reduced). \(O_2\) (oxidation state \(0\)) to \(O^{2 -}\) (oxidation state \(-2\)) in \(Fe_2O_3\). So \(O_2\) is the oxidizing agent.
• Reducing agent: Substance that loses electrons (is oxidized). \(Fe\) (oxidation state \(0\)) to \(Fe^{3+}\) (oxidation state \(+3\)) in \(Fe_2O_3\). So \(Fe\) is the reducing agent.

Answer:

Oxygen has an oxidation state of - 2 in \(Fe_2O_3\) (first option).