Cathodic protection of iron involves using another more reactive metal as a sacrificial anode. Classify each of the following metals by whether they would or would not act as a sacrificial anode to iron.

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Ag
Mg
Cu
Pb
Sn
Zn
Au

a. Will act as sacrificial anode for iron
b. Will not act as sacrificial anode for iron

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

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890