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