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CHM135 > electrochemistry > Flashcards

electrochemistry Flashcards

1
Q

electrochemistry is the interconversion of

A

chemical and electrical energy

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2
Q

Spontaneous reactions can produce electricity and power

A

power a nonspontaneous reaction to occur

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3
Q

Oxidation means loss of

A

electrons

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4
Q

Reduction is the gain of

A

electrons

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5
Q

whats oil rig

A

Oxidation Is Loss ELECTRONS

Reduction Is gain ELECTRONS

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6
Q

redox reactions involve movement of _______ from one _______ to another

A

electrons

reagent

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7
Q

WHAT DOES O2 FREQUENTLY ACT AS

A

an oxidizing agent

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8
Q

Steps for balancing reagents

A
  1. write down two half-reactions containin
  2. balance atoms and charges
  3. electrons should cancel out
  4. add the balanced half reactions
  5. check both charges balance
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9
Q

Two types of voltaic cells

A

voltaic cell

electrolytic cell

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10
Q

Voltaic/galvantic cells are

A

spontaneous chemical reaction generates an electric current

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11
Q

electrolytic cells are….

and they have to be ……..

A

non-spontaneous reactions are driven by electric current

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12
Q

what things typically contains voltaic/galvantic cells

A

batteries

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13
Q

does Voltaic cell system do work on surrounding or does surrounding do work on it? how>

A

yes it does work on the surroundings

by converting high energy in reactants in cell to lower energy products

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14
Q

does electrolytic cell system do work on surrounding or does surrounding do work on it? how?

A

the surrounding does work on the electrolytic cell system

Lower energy reactants are converted to higher energy products in ce;;

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15
Q

Voltaic cells use _____ reactions (G ___ 0) to do generate electrical energy

A

spontaneous

G < 0

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16
Q

salt in salt bridge go towards

A

reduction

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17
Q

Electric current is

A

flow of electrons

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18
Q

electrons only flow if the ____. force is large enough

A

driving

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19
Q

Anode is the electrode where

A

oxidation happens

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20
Q

cathode is the electode where

A

reduction happens

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21
Q

red cat means

A

reduction is cathode

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22
Q

electrodes are _____ strips connected by an _____ conducting wire

A

metal

electrically

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23
Q

salt bridge: _ shaped tube contains a ___ ____________ solution of an ________ electrolyte

A

U

gel permeated

inert

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24
Q

What does salt bridge do

A

keeps half cells electrically neutral as ions flow in and out

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25
Q

Voltaic cell notation

anode

cathode

A

Anodes are on the left

cathodes on the right

26
Q

Voltaic cell notation

the order of written half cell

A

written in same order that would appear in their own half cell rxns

27
Q

voltaic cell notation

double line

A

means that half-cells are physically separated

28
Q

voltaic cell notation

if needed concentrations..

if not given concentration

A

it would be in brackets

assume 1M

29
Q

voltaic cell notation

direction of electron flow

A

——–>

30
Q

voltaic cell notation

comma

A

shows components taht are in the same phase

31
Q

voltaic cell notation

“graphite”

A

shows any inactive (inert) electrode

32
Q

Differing abilities of the metals to gain electrons gives rise to a ____ _____. Known as __________ ____ (EMF) or cell potential

A

voltage drop

electromotive force

33
Q

multimeter measures

A

voltage

34
Q

Cell potential (Ecell) is the

A

difference in electrical potential between two electrodes

35
Q

if Ecell > 0 for VOLTAIC CELLS

A

spontaneous

36
Q

if Ecell < 0 for ELECTROLYTIC CELLS

A

non spontaneous

37
Q

Ecell bigger general formula

A

Eoxidation + Ereduction

38
Q

Are half cell potentials multiplied

A

no

39
Q

Lower Ecell voltage is always

A

flipped sign

40
Q

whats S.H.E stand for. what is it

A

standard hydrogen electrode

reference point

41
Q

potentials are determined experimentally from the _______ in potential

A

difference

42
Q

S.H.E arbitraty value of

A

0.00V

43
Q

how is Ecell related to thermodynamic property

A

negative

44
Q

way to determine equilibrium constant for redox

A

-nFEcell = ΔG° = -RTlnK

45
Q

ECELL (draw triagnle)=

A

(RT/NF) x lnK

46
Q

K from equilibrium concentration/ partial pressures

A

k = [C]ᶜ[D]ᵈ/ [A]ᵃ[B]ᵇ

47
Q

K FOR STANDARD STATE THEROMCEMIAL

A

lnk = -ΔG°/RT

48
Q

K for standard state electrochemical data IF EQUILIBRIUM INVOLVED REDOX REACTION

also what else need to remember?

A

lnK = nFE°cell/RT

account for the amount of charge transferred

49
Q

Nernst equation

A

E= E° - RT/nF lnQ

50
Q
A
51
Q

cell potential depends on relative …

A

concentrations of reactants and products

52
Q

When Q < 1, ln Q < 0, so E cell…..

when Q = 1, ln Q = 1, so E cell…..

When Q > 1, ln Q > 0, so E cell….

A

E cell > E°

E cell = E°

E cell < E°

53
Q

As cell is operated, concentrations of reactants will decrease and products will increase, but overall, this consequence of cell potential is

A

the overall cell potenetial decrease over time

54
Q

what do concentration cells capture

A

electrical energy from concentration difference when

55
Q

E cell =. (cathode and anote way_

A

E cell = E cathode - E anode

56
Q

a concentration cell _____ the effect of concentration differences.

A

EXPLOITS

57
Q

E cell > 0 as long as the half-cell concentrations are

A

different

58
Q

Once concentrations in concentration cells equalize, ____ = _____ and current stops ______

A

Ecell = 0

flowing

59
Q

Galvanization is

A

coating of iron with zinc

60
Q

at 25C, what altnerate form can i use to find equilibrium constant

A

logK = nEcell/0.0592

CHM135 (8 decks)

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