Electrochemistry Flashcards

1
Q

oxidation

A

loss of electrons

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2
Q

reduction

A

gain of electrons

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3
Q

what agent is the oxidized atom

A

reducing agent

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4
Q

what agent is the reduced atom

A

oxidizing agent

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5
Q

what happens at anode

A

oxidation

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6
Q

what happens at cathode

A

reduction

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7
Q

galvanic cell function

A

flow of electrons create an electric current that can do work in a redox reaction. spontaneous redox reactions generate electric currents

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8
Q

anode

A

electron source

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9
Q

cathode

A

electron sink

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10
Q

how do electrons flow in galvanic cell

A

anode to cathode

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11
Q

salt bridge anion and cation destinations

A

anion goes to anode, cation goes to cathode

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12
Q

what do salt bridges complete

A

circuit

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13
Q

what are the standard conditions

A

25 degrees celcius, 1 atm, 1 M

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14
Q

what is free energy change for a redox reaction?

A

delta G = -nFE

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15
Q

What must cell voltage and free energy be to be spontaneous

A

cell voltage positive, free energy negative

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16
Q

If a reduction potential is negative, what are characteristics of reactant

A

better as a reducing agent, weak oxidizing agent

17
Q

if a reduction potential is positive, what are characteristics of reactant

A

stronger as an oxidizing agent and weaker as a reducing agent

18
Q

What are nonstandard conditions

A

when solution does not equal 1 M and nernst equation must be used

19
Q

concentration cell

A

galvanic cell with identical electrodes but has half cells with different ion concentrations

20
Q

what is anode in concentration cell

A

lower concentration solution

21
Q

what is cathode in concentration cell

A

higher concentration solution

22
Q

when does reaction stop in concentration cell

A

when concentrations are equal

23
Q

what is standard cell voltage in concentration cell

A

zero, since ions in two beakers have same identities

24
Q

redox indicator

A

uses change in color to determine endpoint. change is due to change in oxidation state

25
what makes a redox indicator an ideal indicator
having a high redox potential for determination of solution with oxidizable species
26
At half equivalence point
oxidized and non oxidized are equal and Q = 1. E= E prime
27
Electrolytic Cells
Use external voltage (battery) to create electric current that forces nonspontaneous reactions to occur.
28
Electrolysis
use of electrolytic cells
29
Electroplating
electrolytic cells are used for plating thin layer of metal on top of another material
30
Anode in electrolytic cells charge
positive, because electrons are forced to move
31
Cathode in electrolytic cells charge
negative, because electrons are forced to move
32
Faraday's Law of electrolysis
amount of chemical charge is proportional to amount of electricity that flows through cell
33
Faraday
magnitude of charge on 1 mole of electrons