Electrochemistry (5/16) Flashcards

1
Q

Standard reduction potential

A

E0
measured in volts
used to refer to any reduction half-reaction

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2
Q

More positive reduction potential

A

likes to be reduced, more spontaneous

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3
Q

Electrochemical cell

A

uses electric energy to make a reduction reaction happen

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4
Q

Anode

A

site of oxidation

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5
Q

Catode

A

site of reduction

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6
Q

Galvanic cells

A

A spontaneous reaction is used to generate a positive potential difference that drives a current
E0 must always be positive

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7
Q

Finding reaction direction in a galvanic cell 1

A

1: identify which reaction happens at the cathode and which happens at the anode, reverse the half reaction at the anode and flip its sign and add potentials

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8
Q

Finding reaction direction in a galvanic cell 2

A

2: identify which reaction happens at the cathode and which happens at the anode, Ecell= Ecathode- Eanode to find the different in reduction potential

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9
Q

Daniell cell

A

two half cells connected by a wire and a salt bridge

ions can travel back and fourth

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10
Q

Concentration cell

A

electrodes must be the same material
two regions must have concentration difference
anode to cathode

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11
Q

Electrolytic cells

A

electrical energy is used to drive a non-spontaneous redox reaction
negative E0

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12
Q

Electroplating

A

non-spontaneous reduction of metal ion in solution
results in a deposition of solid metal onto cathode
mol=IT/nF
current*time/ mole e- * Faraday’s constant

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13
Q

Rechargeable batteries

A

Can either discharge (galvanic)spontaneously or recharge (electrolytic), allowing multiple uses

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14
Q

Lead acid battery

A

has a relatively low energy density or low energy to mass ratio
used in some applications today

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15
Q

Nickle cadium

A

cathode and anode

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16
Q

Nerst equation

A

helps account for how electrical potential of a cell is affected by temperature and concentration of reactants
E’cell=Ecell-RT/zF*LnQ

17
Q

Nerst equation simplified

A

E’cell=E0cell-0.05916/z*logQ

18
Q

When products increase

A

lower E, more non-spontaneous

19
Q

Thermodynamics

A

-nFE0cell