electrochemistry lesson 7 the standard hydrogen cell
DESCRIPTION
Electrochemistry Lesson 7 The Standard Hydrogen Cell. The Standard Hydrogen Half Cell The zero point of the reduction chart is the hydrogen half-cell. E is the cell potential or voltage E 0 is the standard cell potential @ 25 o C solutions are 1.0 M gases are 101 KPa. - PowerPoint PPT PresentationTRANSCRIPT
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ElectrochemistryLesson 7
The StandardHydrogen Cell
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The Standard Hydrogen Half Cell
The zero point of the reduction chart is the hydrogen half-cell.
E is the cell potential or voltage
E0 is the standard cell potential @ 25 oCsolutions are 1.0 Mgases are 101 KPa
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Ag+ reacts with H2 spontaneously Eo = +0.80 v
Zn2+ is nonspontaneous with H2 Eo = -0.76 v
All half reactions are compared to H2
The voltage for any combination is the difference
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Using the Reduction Potential Chart
Look on your reduction chart to find the voltage of each agent. Oxidizing agents are on the left and reducing agents are on the right. Formula Agent Type E0
HClO4 oxidizing
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Using the Reduction Potential Chart
Look on your reduction chart to find the voltage of each agent. Oxidizing agents are on the left and reducing agents are on the right. Formula Agent Type E0
ClO4
- Acid oxidizing 1.39 v
HNO3 oxidizing
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Take higher oneStronger Oxidizing Agent
HNO3 is both H+ and NO3
-
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Using the Reduction Potential Chart
Look on your reduction chart to find the voltage of each agent. Oxidizing agents are on the left and reducing agents are on the right. Formula Agent Type E0
ClO4
- Acid oxidizing 1.39 v
HNO3 oxidizing 0.96 v
HCl oxidizing
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Using the Reduction Potential Chart
Look on your reduction chart to find the voltage of each agent. Oxidizing agents are on the left and reducing agents are on the right. Formula Agent Type E0
ClO4
- Acid oxidizing 1.39 v
HNO3 oxidizing 0.96 v
HCl oxidizing 0.00 vSO4
2- reducing
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The reaction is reversed so the E0 = -2.01 v
Oxidation
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Using the Reduction Potential Chart
Look on your reduction chart to find the voltage of each agent. Oxidizing agents are on the left and reducing agents are on the right. Formula Agent Type E0
ClO4
- Acid oxidizing 1.39 v
HNO3 oxidizing 0.96 v
HCl oxidizing 0.00 vSO4
2- reducing -2.01 v
MnO4- Acid oxidizing
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Using the Reduction Potential Chart
Look on your reduction chart to find the voltage of each agent. Oxidizing agents are on the left and reducing agents are on the right. Formula Agent Type E0
ClO4
- Acid oxidizing 1.39 v
HNO3 oxidizing 0.96 v
HCl oxidizing 0.00 v SO4
2- reducing -2.01 v
MnO4- Acid oxidizing 1.51 v
MnO4- Alkaline oxidizing
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Using the Reduction Potential Chart
Look on your reduction chart to find the voltage of each agent. Oxidizing agents are on the left and reducing agents are on the right. Formula Agent Type E0
ClO4
- Acid oxidizing 1.39 v
HNO3 oxidizing 0.96 v
HCl oxidizing 0.00 vSO4
2- reducing -2.01 v
MnO4- Acid oxidizing 1.51 v
MnO4- Alkaline oxidizing 0.60 v
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Formula Agent Type E0
H2SO4 oxidizing
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H2SO4 → HSO4- + H+
Don’t have SO42-
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Formula Agent Type E0
H2SO4 oxidizing 0.00 v
H2O Neutral oxidizing
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Formula Agent Type E0
H2SO4 oxidizing 0.00 v
H2O Neutral oxidizing -0.41 v
H2O Neutral reducing
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Formula Agent Type E0
H2SO4 oxidizing 0.00 v
H2O Neutral oxidizing -0.41 v
H2O Neutral reducing -0.82 v
Fe2+ reducing
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Formula Agent Type E0
H2SO4 oxidizing 0.00 v
H2O Neutral oxidizing -0.41 v
H2O Neutral reducing -0.82 v
Fe2+ reducing -0.77 v
Fe2+ oxidizing
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Formula Agent Type E0
H2SO4 oxidizing 0.00 v
H2O Neutral oxidizing -0.41 v
H2O Neutral reducing -0.82 v
Fe2+ reducing -0.77 v
Fe2+ oxidizing -0.45 v
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Determine if the reaction below is spontaneous. Write a balanced equation for the reaction and calculate the E0. 1. MnO4
- & Mn2+ Acid
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Reduction
Oxidation
The top reaction is written forward
The bottom reaction is reversed and the voltage is changed to negative
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Determine if the reaction below is spontaneous. Write a balanced equation for the reaction and calculate the E0. 1. MnO4
- & Mn2+ Acid
2(MnO4- + 8H+ + 5e-→ Mn2+ + 4H2O) 1.51 v
5(Mn2+ + 2H2O → MnO2(s)+ 4H+ + 2e-) -1.22 v
2MnO4-+16H++5Mn2++10H2O → 2Mn2++8H2O+5MnO2(s)+20H+
2MnO4- + 3Mn2+ + 2H2O → 5MnO2(s) + 4H+ 0.29 v
add potentials
40.29 v
3 2
simplify
positive voltage- spontaneous