Question

decide whether each chemical reaction in the table below is an oxidation - reduction (
edox\) reaction. if the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent.

2cl₂(g)+sn(s)→sncl₄(s)

co₂(g)+2h₂o(l)→h₃o⁺(aq)+hco₃⁻(aq)

fe(s)+cuso₄(aq)→feso₄(aq)+cu(s)

Explanation:

Step1: Determine oxidation states

• For \(2Cl_{2}(g)+Sn(s)\to SnCl_{4}(s)\):
• In \(Cl_{2}\), oxidation state of \(Cl\) is \(0\). In \(SnCl_{4}\), oxidation state of \(Cl\) is \(- 1\).
• In \(Sn\), oxidation state of \(Sn\) is \(0\). In \(SnCl_{4}\), oxidation state of \(Sn\) is \(+4\).
• Since there are changes in oxidation states (\(Cl\) is reduced from \(0\) to \(-1\), \(Sn\) is oxidized from \(0\) to \(+4\)), it is a redox reaction.
• The reducing agent is \(Sn\) (it donates electrons and gets oxidized).
• The oxidizing agent is \(Cl_{2}\) (it accepts electrons and gets reduced).

Step2: Analyze \(CO_{2}(g)+2H_{2}O(l)\to H_{3}O^{+}(aq)+HCO_{3}^{-}(aq)\)

• Calculate oxidation states:
• In \(CO_{2}\), \(C\) is \(+4\), \(O\) is \(-2\). In \(H_{2}O\), \(H\) is \(+1\), \(O\) is \(-2\). In \(H_{3}O^{+}\), \(H\) is \(+1\), \(O\) is \(-2\). In \(HCO_{3}^{-}\), \(H = + 1\), \(C=+4\), \(O=-2\).
• There are no changes in oxidation states. So it is not a redox reaction.

Step3: Examine \(Fe(s)+CuSO_{4}(aq)\to FeSO_{4}(aq)+Cu(s)\)

• Determine oxidation states:
• In \(Fe\), oxidation state of \(Fe\) is \(0\). In \(FeSO_{4}\), oxidation state of \(Fe\) is \(+2\).
• In \(CuSO_{4}\), oxidation state of \(Cu\) is \(+2\). In \(Cu\), oxidation state of \(Cu\) is \(0\).
• Since there are changes in oxidation states (\(Fe\) is oxidized from \(0\) to \(+2\), \(Cu\) is reduced from \(+2\) to \(0\)), it is a redox reaction.
• The reducing agent is \(Fe\) (it donates electrons and gets oxidized).
• The oxidizing agent is \(CuSO_{4}\) (it accepts electrons and gets reduced).

Answer:

For \(2Cl_{2}(g)+Sn(s)\to SnCl_{4}(s)\):

• redox reaction? yes
• reducing agent: \(Sn\)
• oxidizing agent: \(Cl_{2}\)

For \(CO_{2}(g)+2H_{2}O(l)\to H_{3}O^{+}(aq)+HCO_{3}^{-}(aq)\):

• redox reaction? no

For \(Fe(s)+CuSO_{4}(aq)\to FeSO_{4}(aq)+Cu(s)\):

• redox reaction? yes
• reducing agent: \(Fe\)
• oxidizing agent: \(CuSO_{4}\)