Respuesta :
Answer:
Explanation:
Materials used for sacrificial anodes must be relatively pure active metals.
Or we can say any metal with more negative potential that that of iron ( +0.59) is used for sacrificial anode for iron
so from the above the following can be used as sacrificial anode for iron
Mg = +1.06
Al = +0.96
Zn = +0.7
The following will not be used as sacrificial anode for iron because their negative reduction potential is less than that of iron ( +0.59)
Ag = -0.76
Cu = -0.44
Pb = 0
Sn = +0.34
Au = -3.05
Part a. Ag ---> They cannot serve as a sacrificial anode for iron because it is lower than iron in the reactivity series. Hence proof, it is less reactive than iron.
Part b. Mg ---> They can serve as a sacrificial anode for iron because it is higher than iron in the reactivity series. Hence proof, it is more reactive than iron.
Part c. Cu ---> They cannot serve as a sacrificial anode for iron because it is lower than iron in the reactivity series. Hence proof, it is less reactive than iron.
Part d. Pb ---> They cannot serve as a sacrificial anode for iron because it is lower than iron in the reactivity series. Hence proof, it is less reactive than iron.
Part e. Sn ---> They can't serve as a sacrificial anode for iron because it is lower than iron in the reactivity series. Hence proof, it is less reactive than iron.
Part f. Zn ---> They can serve as a sacrificial anode for iron because it is higher than iron in the reactivity series. Hence proof, it is more reactive than iron.
Part g. Au ---> They cannot serve as a sacrificial anode for iron because it is lower than iron in the reactivity series. Hence proof, it is less reactive than iron.
What is a Cathodic protection of iron?
Materials are used for sacrificial anodes must be relatively pure active metals. or we can say that any metal with more negative potential than iron ( +0.59) is used for sacrificial anode for iron
After that, from the above, the following can be used as a sacrificial anode for iron is:
Mg is = +1.06
Al is = +0.96
Zn is = +0.7
The following as given will not be used as a sacrificial anode for iron just because their negative reduction potential is less than that of iron ( +0.59)
Ag is = -0.76
Cu is = -0.44
Pb is = 0
Sn is = +0.34
Au is = -3.05
When the Cathodic protection of iron is involved using another more reactive metal as a sacrificial anode. Then The reactivity series of metals arranges metals based on decreasing order of reactivity. After that, The more reactive metals are found higher up in the series while the least reactive metals are found at the lower ends of the series. Thus, metals above iron in the reactivity series can serve as sacrificial anodes by protecting against corrosion, while those lower than iron cannot.
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