Using the following portion of the activity series for oxidation half reactions K(s)→ K⁺(aq)+ e^- Al(s)→ Al³⁺(aq)+ 3e^- Fe(s)→ Fe²⁺(aq)+ 2e^- Sn(s)→ Sn²⁺(aq)+ 2e^- Determine which pairs of reactions will occur. A)Al(s)with Fe²⁺(aq)and Sn(s)with K⁺(aq) B)Fe(s)with Al(s)and Al³⁺(aq)with Sn²⁺(aq) C)Fe(s)with Sn²⁺(aq)and Al(s)with Sn²⁺(aq) D)K(s)with Al³⁺(aq)and Fe(s)with Al³⁺(aq)

Question

Quizplus · Accepted Answer

In order for a reaction to occur, the metal in the oxidation half reaction needs to be higher on the activity series than the metal in the reduction half reaction. In option A, Al is higher on the activity series than Fe, but Sn is not higher on the activity series than K, therefore, only the reaction between Al and Fe will occur. In option B, Fe is higher on the activity series than Al, but Sn is not higher on the activity series than Al, therefore, only the reaction between Fe and AlS1U1P13 will occur. In option D, K is higher on the activity series than Al, but Fe is not higher on the activity series than Al, therefore, neither reaction will occur. However, in option C, Fe is higher on the activity series than Sn and Al is higher on the activity series than Sn, therefore, both reactions will occur.

Using the Following Portion of the Activity Series for Oxidation