Question

Write the oxidation, reduction, and redox reactions for:

a) silver (Ag) reacting with Cu(NO3)2 (Why is it that no reaction occurs here?)

b) copper (Cu) reacting with Mg(NO3)2 (Why is it that no reaction occurs here?)

c) zinc (Zn) reacting with Pb(NO3)2

d) lead (Pb) reacting with AgNO3

e) magnesium (Mg) reacting with NaCl (Why is it that no reaction occurs here?)

Please show ALL steps and explanations. Thank you.

Answer 1

(a)

No reaction occurs because reduction potential of silver is greater than that of copper, so it will not get oxidized to replace Cu²⁺.

(b)

No reaction occurs because reduction potential of copper is greater than that of magnesium, so it will not get oxidized to replace Mg²⁺.

(c)

The balanced reaction is:

Zn(s) + Pb(NO₃)₂ ---> Zn(NO₃)₂ + Pb(s)

(d)

The balanced reaction is:

Pb(s) + 2AgNO₃ ---> Pb(NO₃)₂ + 2Ag(s)

(e)

No reaction occurs because both MgCl₂ and NaCl are completely soluble, so no precipitate formation takes place.

Hope this helps !