Question

Write the oxidation, reduction, and redox reactions for:

a) silver (Ag) reacting with Cu(NO3)2

b) copper (Cu) reacting with Mg(NO3)2

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

d) lead (Pb) reacting with AgNO3

e) magnesium (Mg) reacting with NaCl

Please show ALL steps. Thank you.

Answer 1

a) silver (Ag) reacting with Cu(NO3)2

Ag(s) + Cu(NO3)2 (aq) --------------------> No reaction

b) copper (Cu) reacting with Mg(NO3)2

Cu(s) + Mg(NO3)2 (aq) ------------------> No reaction

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

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

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

removal of spectator ions to get net ionic equation

Zn(s) + Pb^2+ (aq) -----------------> Zn^2+ (aq)+ Pb(s)

Zn(s) -----------------------> Zn^2+ (aq) + 2e^-   oxidation

Pb^2+ (aq) + 2e^- -----------> Pb(s) reduction

-------------------------------------------------------------------------

Zn(s) + Pb^2+ (aq) -----------------> Zn^2+ (aq)+ Pb(s) redox reaction

d) lead (Pb) reacting with AgNO3

Pb(s) + 2AgNO3(aq) ---------------------> Pb(NO3)2(aq) + 2Ag (aq)

Pb(s) + 2Ag^+ (aq) +2NO3^-(aq) ---------------------> Pb^2+ (aq) +2(NO3)^-(aq) + 2Ag (aq)

removal of spectator ions to get net ionic equation

Pb(s) + 2Ag^+ (aq) ---------------------> Pb^2+ (aq) + 2Ag (aq)

Pb(s) -----------------------> Pb^2+ (aq) + 2e^-        oxidation

2Ag^+ (aq) + 2e^- -----------------> 2Ag(s)             reduction

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Pb(s) + 2Ag^+ (aq) ---------------------> Pb^2+ (aq) + 2Ag (aq) redox rection

e) magnesium (Mg) reacting with NaCl

Mg(s) + NaCl (aq) ---------------------------> No reaction