Zn │ Zn 2+ ││Cu 2+ │ Cu Std Electromotive Force = Std EMF = Std Cell potential = E° = 1.10 V 2H + + 2e - → H 2 (at 1 atm, 1 M, 25°) Standard EMF = 0 (E°

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Presentation transcript:

Zn │ Zn 2+ ││Cu 2+ │ Cu Std Electromotive Force = Std EMF = Std Cell potential = E° = 1.10 V 2H + + 2e - → H 2 (at 1 atm, 1 M, 25°) Standard EMF = 0 (E° 2H + →H 2 =0)

Zn 2+ H+H+ 1 M ZnSO 4 1 M HCl Zn Pt 1 Atm H 2(g) voltmeter 0.76 V KNO 3 Zn Zn 2+ H +, H 2 Pt

1M Ag + 1 M Cl - Ag Pt 1 Atm Cl 2(g) voltmeter 0.56 V KNO 3 Ag + + 1e - → Ag Cl 2 + 2e - → 2Cl - 2 Ag + Cl 2 → 2Cl - + 2Ag + Complete standard cell with all noteworthy parts labeled. Half reactions shown at appropriate location Overall reaction. Voltage on meter. Show the proper line notation. Salt bridge Ag →Ag e - Cl 2 + 2e - →2Cl - Ag Ag + Cl 2, Cl - Pt ←anode ←cathode E° = 1.36 V E° = 0.80 V 2( )