writing net-ionic equations...net ionic equation for silver lab (without spectator ions) cu (s) +...

Chemical Equation for Silver lab

Cu (s) + 2AgNO3 (aq) 2Ag (s) + Cu(NO3)2 (aq) Ionic Equation for Silver Lab (with Spectator Ions) Cu (s) + 2Ag1+ (aq) + 2NO3

1- (aq) 2Ag (s) + Cu2+ (aq) + 2NO31- (aq)

Net Ionic Equation for Silver Lab (without Spectator Ions) Cu (s) + 2Ag1+ (aq) 2Ag (s) + Cu2+ (aq)

Writing Net-Ionic Equations

Net-Ionic Equation

Spectator Ions

Anode Cathode

Cu0 Cu2+ + 2e- Ag1+ + 1e- Ag0

Anode Cathode

Cu0 Cu2++ 2e- Ag1+ + 1e-

Ag0

Eo = -0.34 V Eo = +0.80 V

Oxidation Process Reduction Process

Reducing Agent Oxidizing Agent

Cu(s) | Mg2+ (1.0 M) || Ag1+(1.0 M) | Ag (s)

Eocell = +0.46 V

Anode Cathode

Zn0 Zn2+ + 2e- Ag1+ + 1e- Ag0

The short-hand chemistry notation used to represent the electrochemical cell redox

reaction shown in the previous illustration is written as

Zn (s) | Zn2+ (1.0 M) || Cu2+ (1.0 M) | Cu (s)

By convention, the half-cell with the anode, undergoing oxidation, is placed to the left.

The half-cell with the cathode, undergoing reduction, is placed to the right of the

double-vertical line. The standard-state ion concentrations are 1-M concentrations.

Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V

Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V

Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V

Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V

Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V

Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V

Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V

Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V

Cu2+ (aq) + 2e- = Cu (s) Eo oxidizing agent = +0.34 V

Zn(s) = Zn2+ (aq) + 2e- Eo reducing agent = +0.76 V

Cu2+(aq) + 2e- = Cu(s) Eooxidizing agent = +0.34 V

Zn(s) = Zn2+(aq) + 2e- Eoreducing agent = +0.76 V

_____________________________________________________

Cu2+(aq) + Zn(s) = Cu(s) + Zn2+(aq) DEocell = +1.10 V

Zn (s) | Zn2+ (1.0 M) || Cu2+(1.0 M) | Cu (s)

Anode Cathode

Oxidation Reduction

Reducing Agent Oxidizing Agent

__ (s) | ____ (1.0 M) || ____(1.0 M) | __ (s)

Anode Cathode

Oxidation Reduction

Reducing Agent Oxidizing Agent

2Ag1+(aq) + 2e- = 2Ag(s) Eooxidizing agent = _____V

__(s) = Zn2+(aq) + 2e- Eoreducing agent = _____V

_____________________________________________________

2Ag1+(aq) + Zn(s) = Zn2+(aq) + 2 __(s) DEocell = ______V

Zn(s) | Zn2+ (1.0 M) || Ag1+(1.0 M) | Ag (s)

Anode Cathode

Oxidation Reduction

Reducing Agent Oxidizing Agent

2Ag1+(aq) + 2e- = 2Ag(s) Eooxidizing agent = +0.80 V

Zn(s) = Zn2+(aq) + 2e- Eoreducing agent = +0.76 V

_____________________________________________________

2Ag1+(aq) + Zn(s) = Zn2+(aq) + 2Ag(s) DEocell = +1.56 V

Cu2+(aq) + 2e- = Cu(s) Eooxidizing agent = +0.34 V

Zn(s) = Zn2+(aq) + 2e- Eoreducing agent = +0.76 V

_____________________________________________________

Cu2+(aq) + Zn(s) = Cu(s) + Zn2+(aq) DEocell = +1.10 V

2Ag1+(aq) + 2e- = 2Ag(s) Eooxidizing agent = +0.80 V

Zn(s) = Zn2+(aq) + 2e- Eoreducing agent = +0.76 V

_____________________________________________________

2Ag1+(aq) + Zn(s) = Zn2+(aq) + 2Ag(s) DEocell = +1.56 V

+0.34 V

+0.80 V

-0.76 V

Eohalf cell

Zn(s) | Zn2+ (1.0 M) || Ag1+(1.0 M) | Ag (s)

Anode Cathode

Oxidation Reduction

Reducing Agent Oxidizing Agent