Question

Reduction occurs, the electrode is negative and iron metal is formed. QUESTION 10 Which of the following metals would slow down the rate of corrosion of iron metal if placed in electrical contact with the iron? Note that this is a multiple answer question, you can select more than one answer. Mg(s) Ag(s) Al(s) Sn(s) Cu(s) QUESTION 11 Match the voltaic and electrolytic cell concepts A. 4 Requires energy input A. Electrolytic

Answer 1

Look at the electrochemical series. The elements present at the top of the table are most oxidising and elements present at the below are most reducing. Here corrosion of iron means conversion of Fe to Fe2+ (oxidation).

To get the correct answer to this problem, we need to first locate the position of Fe2+/Fe in the electrochemical series and then look at the metals present above and below to that of iron. The metals above iron will have more oxidising property and will easily oxidise iron and thus increase the rate of corrosion. On the other hand, metals below iron will not have enough oxidising property to oxidise Fe to Fe2+. Thus metals below iron in the series will slow down the rate of corrosion.

By looking at the table we can see-

Ag, Sn, Cu are present above iron in the series.

Mg and Al are present below iron in the series.

So correct option is Mg and Al.