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Unit 3 - Electrochemistry > Chapter 14 - Electrochemical Cells > Flashcards

Chapter 14 - Electrochemical Cells Flashcards

1
Q

Why are electric vehicles better than gas ones?

A

Because they are more efficient and create less pollution. They are also nearly silent and don’t need too much maintenance.

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2
Q

What is the main reason that electric cars aren’t around yet?

A

There is no powerful, lightweight, inexpensive battery.

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3
Q

Who invented the first electric cell?

A

Volta, inspired by Galvani.

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4
Q

What does an electric cell do?

A

Converts chemical energy into electrical energy.

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5
Q

What is a battery?

A

A group of two or more cells.

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6
Q

What is brine?

A

Aqueous sodium chloride.

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7
Q

What was Volta’s first battery like?

A

It was bowls of brine with copper and zinc connected going through each one. Then it was layers of copper, paper soaked in salt solution, and then zinc (a voltaic pile).

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8
Q

Basic components of an electric cell:

A

Two electrodes and one electrolyte.

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9
Q

What is an electrode?

A

A solid electrical conductor.

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10
Q

What is an electrolyte?

A

Aqueous electrical conductor.

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11
Q

In an electric cell or battery, the _______ is the positive electrode and the ______ is the negative electrode.

A

Cathode; anode.

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12
Q

Electricity is the flow of…

A

Electrons.

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13
Q

Electrons move from the ___ to the ____.

A

Anode to the cathode.

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14
Q

What do the electrons move through?

A

An external circuit like a wire.

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15
Q

What is a voltmeter?

A

Used to measure energy difference between any 2 points in an electric circuit.

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16
Q

What is electrical potential difference?

A

Energy difference per unit charge.

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17
Q

Is voltage effected by the size of a battery or cell?

A

No.

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18
Q

The voltage of a cell mainly depends on:

A

the chemical composition of the reactants in the cell.

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19
Q

Electric current is measured by

A

an ammeter (in amperes).

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20
Q

The larger the electric cell, the greater…

A

the current that can be produced.

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21
Q

The charge transferred by a cell or battery is measured by…

A

Coloumbs.

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22
Q

Power of a cell is measured in…

A

watts.

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23
Q

Energy density is measured as

A

Joules/kilogram

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24
Q

Which came first, the discovery of cells or the discovery of electrons?

A

Cells.

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25
Q

What kind of cell is commonly referred to as a “dry cell?”

A

A zinc chloride cell.

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26
Q

What is a primary cell?

A

A cell that cannot be recharged.

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27
Q

Types of primary cells?

A

Dry cell, alkaline dry cell, mercury cell.

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28
Q

Types of secondary cells?

A

Ni-Cd cell, lead-acid cell.

29
Q

Types of fuel cells?

A

Hydrogen-oxygen cell, aluminium air-cell.

30
Q

How is a secondary cell recharged?

A

Using electricity to reverse the chemical reaction that occurs when electricity is produced by the cell.

31
Q

What type of battery is in a typical car battery?

A

A lead-acid cell.

32
Q

Recharging a cell is not spontaneous because…

A

it takes energy.

33
Q

How does a fuel cell work?

A

They produce electricity by the reaction of a fuel that is continuously supplied to keep the cell operating.

34
Q

Are fuel cells more efficient than methods that produce electricity by the burning of fossil fuels?

A

Yes.

35
Q

Basic description of an aluminium-air cell:

A

Air is pumped in an oxygen is reduced at the cathode while aluminium is oxidized at the anode. Has been developed to be used in electric cars.

36
Q

What are galvanic cells?

A

Cells adapted for scientific study.

37
Q

What is a porous boundary?

A

It separates the two electrolytes in a voltaic cell. Allows ions through, though, through the salt bridge.

38
Q

What does a half-cell consist of?

A

One electrode and one electrolyte.

39
Q

What does a single line (I) represent in cell notation?

A

A phase boundary.

40
Q

What does a double line (II) represent in cell notation?

A

A physical boundary.

41
Q

What does a voltaic cell consist of?

A

Two half cells separated by a porous boundary.

42
Q

The SRA always undergoes an oxidation at the

A

anode.

43
Q

The SOA always undergoes a reduction at the

A

cathode.

44
Q

What does the salt bridge do?

A

It makes sure that the solutions remain electrically neutral by having cations move to the cathode and anions move to the anode.

45
Q

What is an inert electrode and what does it do?

A

An inert electrode is a solid conductor does not interfere or react with the cell reaction. Inert electrodes provide a pace for a location to connect a wire and a surface on which a half reaction can occur. Usually platinum or carbon.

46
Q

Cell notation format:

A

anode I electrolyte II electrolyte I cathode

47
Q

What is a standard cell?

A

A voltaic cell in which each half-cell contains all entities shown in the half reaction at SATP conditions with a concentration of 1.0mol/L for the aqueous solutions.

48
Q

What is the standard cell potential E°?

A

The maximum cell potential difference (voltage) in standard conditions. This is what a voltmeter measures.

49
Q

What is standard reduction potential?

A

The ability of a standard half-cell to attract electrons , thus undergoing reduction.

50
Q

How do you calculate standard cell potential?

A

Cathode - anode

51
Q

What is a reference cell?

A

Hydrogen, at zero volts.

52
Q

If cell potential is positive, the reaction is

A

spontaneous.

53
Q

Does voltage change as a battery gets older?

A

Yes, it decreases.

54
Q

When electrons flow from the anode to the cathode, it is potential energy to…

A

kinetic energy.

55
Q

What sort of placement on a redox table will get a metal oxidized?

A

If it is a strong reducing metal and below any reaction with oxygen.

56
Q

What is required for the corrosion of iron?

A

Oxygen and water.

57
Q

What can accelerate the rusting of iron?

A

Acidic solutions, electrolytes, mechanical stresses, and less active metals. Salt.

58
Q

Cathodic protection

A

Iron is forced to become the cathode by supplying it with electrons using an impressed current (electric current forced to flow to the iron) or a sacrificial anode. (a metal more easily oxidized than iron).

59
Q

Which is spontaneous, an electrochemical cell or an electrolytic cell?

A

Electrochemical.

60
Q

Basic components of an electrolytic cell:

A

Two electrodes, an electrolyte, and a battery.

61
Q

What is electrolysis?

A

The process of supplying electrical energy to force a nonspontaneous reaction to occur.

62
Q

Does an electrolytic cell have a positive or negative cathode?

A

Negative, opposite of an electrochemical cell.

63
Q

The Chloride Analomy

A

Chlorine gas is produced instead of instead of oxygen gas in situations where chloride and water are the only reducing agents present.

64
Q

Chlor-Alkali Process

A

The electrolysis of brine to produce chlorine, hydrogen, and sodium hydroxide. Chlorine here is the reducing agent anode. Water is the cathode.

65
Q

Electrorefining

A

Uses an electrolytic cell to have pure substance build up on the cathode. Copper is reduced at the cathode.

66
Q

Electrowinning

A

Uses an electrolytic cell to reduce metal cations at the cathode.

67
Q

Q =

A

I x T

68
Q

n e- =

A

Q/F

69
Q

Cell stoichiometry - what is the wanted and what is the given?

A

Depends, but it will be found in the half reaction as the coefficient.

Unit 3 - Electrochemistry (2 decks)

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