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Chemistry: Electrode Potentials Part 3

Chemistry40 CardsCreated 2 months ago

This deck covers key concepts related to electrode potentials, including the electrochemical series, measuring emf, and the applications of electrochemical cells.

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The conventional representation of a cell: using what equation can the cell potential be calculated?

E0RHS-E0LHS
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Key Terms

Term
Definition
The conventional representation of a cell: using what equation can the cell potential be calculated?
E0RHS-E0LHS
To measure E0 for ion/ion half cells: what are ion/ion half cells?
Half cells in which both species are aqueous ions
To measure E0 for ion/ion half cells: what must the half cells contain?
Both the oxidised and reduced species
To measure E0 for ion/ion half cells: what electrode is used?
Platinum
The electrochemical series: in what order can the standard electrode potential values determined by measurement against standard hydrogen electrode be placed in?
Numerical order
The electrochemical series: what are all reactions shown as?
Reductions
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Chemistry: Electrode Potentials Part 3
TermDefinition
The conventional representation of a cell: using what equation can the cell potential be calculated?
E0RHS-E0LHS
To measure E0 for ion/ion half cells: what are ion/ion half cells?
Half cells in which both species are aqueous ions
To measure E0 for ion/ion half cells: what must the half cells contain?
Both the oxidised and reduced species
To measure E0 for ion/ion half cells: what electrode is used?
Platinum
The electrochemical series: in what order can the standard electrode potential values determined by measurement against standard hydrogen electrode be placed in?
Numerical order
The electrochemical series: what are all reactions shown as?
Reductions
The electrochemical series: what can we determine by looking at electrochemical series?
Relative reactivity of different species
The electrochemical series: metals react by losing to form _ ions
Losing electrons to form positive ions
The electrochemical series: reactive metals undergo what more readily?
Oxidation
The electrochemical series: the most reactive metals will have the most _ E0 values
Negative
The electrochemical series: the most reactive metals are good _ agents
Reducing
The electrochemical series: the more negative the E0 values the the tendency for the species on the to electrons and be _
The more negative the E0 the greater the tendency for the species on the RHS to lose electrons and be oxidised
The electrochemical series: non metals react by electrons to form ions
Gaining electrons to form negative ions
The electrochemical series: reactive non metals undergo more readily
Reduction
The electrochemical series: the most reactive non metals will have the most _ E0 values
Positive
The electrochemical series: the most reactive non metals are good agents
Oxidising
The electrochemical series: the more positive the E0 the the tendency for the species on the to electrons and be
The more positive the E0 the greater the tendency for the species on the LHS to gain electrons and be reduced
Measuring the emf of an electrochemical cell, required prac: how else can emf be determined other than using hydrogen electrode?
Any two half cells can be connected to generate an emf
Using electrode potentials to predict chemical reactions: what is chemical energy converted to in an electrochemical cell?
Electrical energy
Using electrode potentials to predict chemical reactions: when did the emf drop to 0.00V in an electrochemical cell?
Once the chemicals are used up
Using electrode potentials to predict chemical reactions: how can we predict what reaction occurs?
By looking at the E0 values of the two half cells
Using electrode potentials to predict chemical reactions: which half equation gains electrons and what does this mean?
The half equation with the more positive E0 value gains electrons, so goes forwards
Using electrode potentials to predict chemical reactions: which half equation loses electrons and what does this mean?
The half equation with the more negative E0 value loses electrons, so goes backwards
Using electrode potentials to predict chemical reactions: what must be certified when adding the two half equations together?
Number of electrons lost=number of electrons gained
Change in mass of the electrode: why does the mass of the negative electrode decrease when a current is drawn?
The metal will be oxidised to metal ions
Change in mass of the electrode: what happens to the mass of the positive electrode and why?
Increases as metal ions turn to metal
The effect of concentration on the emf of a cell: what are the values of E0 measured under standard conditions of?
100kPa, 298K, 1 mol dm-3
The effect of concentration on the emf of a cell: what can be used to predict how concentration changes affect EMF?
Le chateliers principle

The effect of concentration on the emf of a cell (eg Zn|Zn2+||Cu2+|Cu): what will happen if [Cu2+]>1moldm3?

  • equilibrium shifts right

  • ECu more negative

  • Cu2+ gains more electrons

  • Ecell will increase- bigger difference in E

The effect of concentration on the emf of a cell (eg Zn|Zn2+||Cu2+|Cu): what will happen if [Cu2+]<1moldm-3?

  • equilibrium shift LHS

  • ECu less positive

  • Cu2+ will gain feevwr electrons

  • Ecell will decrease- cell has smaller difference in E

The effect of concentration on the emf of a cell (eg Zn|Zn2+||Cu2+|Cu): what will happen if [Zn2+]>1mol dm-3?

  • equilibrium will shift RHS

  • EZn less negative

  • Zn will release fewer electrons

  • Ecell will decrease as cell has smaller difference in E

The effect of concentration on the emf of a cell (eg Zn|Zn2+||Cu2+|Cu): what will happen if [Zn2+] < 1moldm-3?

  • equilibrium shift LHS

  • EZn become more negative

  • Zn will release more electrons

  • Ecell will increase as cell has a bigger difference in E

If conditions are no longer standard what is cell potential written as as opposed to E0Cell?
ECell
Limitations of using electrode potentials to predict redox reactions?
Predictions using electrode potentials tell us about equilibrium but not RoR many reactions in laboratory not done under standard conditions- will affect electrode potential values

Commercial applications of electrochemical cells: what 3 main types can cells be divided into?

  • non- rechargeable cells

  • rechargeable cells

  • fuel cells

Non-rechargeable cells: how are they designed to be used only once?
Reactions occurring in cells cannot be reversed
Non-rechargeable cells: what will happen when the chemicals are used up?
The battery will go flat and the emf will fall to 0.00V
Non-rechargeable cells: used in?
Smoke detectors and clocks
Non-rechargeable cells: overall equation of zinc and manganese dioxide cell when it discharged?
2MnO2 + 2H2O + Zn > 2MnO(OH) + 2OH- + Zn2+
Non-rechargeable cells: function of porous separator?
Allows ions to flow