Ag(s)
The iron is oxidized and the silver is reduced.
Iron (Fe) is a metal that can be oxidized by two common ions: copper ions (Cu^2+) and silver ions (Ag^+).
The answer is not c.
Ag+
Ag(s)
Ag(s)
During electroplating silver onto iron, iron gets oxidized to iron ions (Fe^2+ or Fe^3+). This oxidation process is essential for transferring iron atoms from the iron surface to the silver coating during electroplating.
AgAg(s)-
AgNO3
Fe + 3AgNO3 ==> Fe(NO3)3 plus 3Ag The oxidation number of Ag in AgNO3 (on the left side) is 1+ and in Ag (on the right side), it is zero. Thus, in this reaction, silver (Ag) has been reduced.
In the electroplating process, during the oxidation reaction, silver atoms are oxidized to Ag+ ions for silver plating, and iron atoms are oxidized to Fe2+ ions for iron plating. This allows the metal ions to be deposited onto the object being plated.
In this reaction, Ag^+ is the oxidizing agent. It undergoes reduction by accepting electrons from Fe to form silver metal, while Fe gets oxidized to Fe^3+ in the process.
Ag+ (apex)
Fe(s) + 3AgNO3 ---> Fe(NO3)3 + Ag(s) The oxidation # of Ag on the left is 1+ and on the right it is zero. It has gained electrons and has been reduced.
The iron is oxidized and the silver is reduced.
Iron (Fe) is a metal that can be oxidized by two common ions: copper ions (Cu^2+) and silver ions (Ag^+).