Physical Chapter 8: Electrode Potentials & Cells Flashcards

1
Q

What is an electrochemical cell?

A

A system where two different metals dipped in salt solutions of their own ions are connected by a wire.

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2
Q

What two reactions must always take place within an electrochemical cell?

A

Reduction & Oxidation

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3
Q

Are the reactions that occur at each half-cell reversible?

A

Yes

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4
Q

What are the equations at each half-cell in an electrochemical cell?

A

Half-equations

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5
Q

What way will the half equations in an electrochemical cell be written as?

A

Reduction in the forwards direction

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6
Q

What are electrode potentials measured against?

A

Standard Hydrogen Electrodes

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7
Q

What is standard electrode potential defined as?

A

The standard electrode potential of a half-cell is the voltage measured under standard conditions when the half-cell is connected to a standard hydrogen electrode.

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8
Q

What does an electrochemical series tell you?

A

Relative reactivity of metals.

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9
Q

What do more positive electrode potentials mean for the substances involved?

A

The Left-hand substances are more easily reduced
The right-hand substances are more stable

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10
Q

What do more negative electrode potentials mean for the substances involved?

A

The right-hand substances are more easily reduced
The left-hand substances are more stable

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11
Q

How do you use Electrochemical series to calculate standard cell potentials?

A

Ecell = Ereduced - Eoxidised

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12
Q

What are the conventions when drawing an electrode cell diagram?

A

The most negative potential goes on the left
Oxidised forms go in the centre of the diagram
Things in different phases are separated by a single line
Salt bridge is shown by a double line

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13
Q

How can you use electrode potentials to figure out if a reaction will happen?

A

For any feasible reaction, Ecell will be positive.

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14
Q

What are electrochemical cells often used as?

A

Batteries

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15
Q

What does it mean if a battery is rechargeable?

A

A current is supplied to force electrons to flow in the opposite direction & reverse the reactions

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16
Q

What is a fuel cell typically made of?

A

Hydrogen & Oxygen

17
Q

What is different about a fuel cell compared to electrochemical cells?

A

Chemicals are stored outsde the cell

18
Q

What material do you make the electrode out of when the chemical is gaseous?

A

Platinum

19
Q

Why do you use Platinum for electrodes when chemicals are gaseous?

A

It’s inert

20
Q

What is the electrolyte made of in a Hydrogen-Oxygen fuel cell?

A

KOH - Potassium hydroxide

21
Q

What is an advantage of a fuel cell?

A

They’re more efficient
Only waste produce is water - no greenhouse gases
Don’t need to be recharged

22
Q

What is a disadvantage of a fuel cell?

A

You need energy to produce a supply of hydrogen & oxygen
Hydrogen is highly flammable - handle with care