In an expanded redox activity series, aluminum is located above iron. Which stat

Question

In an expanded redox activity series, aluminum is located above iron. Which statement correctly predicts what will happen (or not happen) when these two metals and its cations interact? Aluminum will act as the stronger reducing agent and iron will act as the stronger oxidant. In the spontaneous reaction, the oxidation number of iron will increase. Aluminum will act as the stronger reducing agent and iron metal ion will act as the stronger oxidant. In the nonspontaneous reaction, the metals will not react because iron is a stronger reducing agent than aluminum. Iron will act as the stronger reducing agent and aluminum will act as the stronger oxidant. In the spontaneous reaction, the oxidation number of aluminum will decrease.

Explanation / Answer

if Al is above Fe, it must be more reactive, i.e. least potential of reduction.

iron is stronger oxidizing agent

iron is reduced, so red ox number decreases

choose the second option, it is the only one suitable in all cases

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