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Chemistry > Unit 3- Electrochemical Cells > Flashcards

Unit 3- Electrochemical Cells Flashcards

1
Q

Are the strongest reducing agents positive or negative?

A

Negative

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2
Q

Define the standard electrode potential of a half-cell (Eθ)?

A

The standard electrode potential of a half-cell is the voltage of a half-cell compared with a standard hydrogen electrode.

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3
Q

Eo values are measured under specific conditions. What are they?

A

1M concentration of electrolyte, 298K and 1 atmosphere

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4
Q

How is the potential cell difference of a galvanic cell calculated?

A

By subtracting the cell potential of the anode from the cathode, the cell potential of the galvanic cell as a whole can be calculated. E0 = E0 reduction - E0 oxidation

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5
Q

In a Galvanic cell, what charge does the anode have?

A

Negative

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6
Q

In an electrolytic cell what charge does the anode have?

A

The anode has a positive charge.

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7
Q

In an electrolytic cell what charge does the anode have?

A

positive

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8
Q

Name the two types of electrochemical cells.

A

Galvanic and electrolytic

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9
Q

Standard electrode potentials are generally written as?

A

Reduction half equation

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10
Q

What are electrolytes?

A

An ionic substance which is either molten or an aqueous solution

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11
Q

What are Eo values?

A

The symbol represents the Cell Potential. It shows the voltage produced in a Galvanic half-cell.

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12
Q

What are galvanic cells used for?

A

Source of electrical energy, batteries

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13
Q

What are standard conditions under which standard electrode potentials are measured?

A

250C, 1 atm and 1M

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14
Q

What are the units for standard electrode potentials?

A

Volts (V)

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15
Q

What charge does the cathode have in an electrolytic cell?

A

The cathode has a negative charge in electrolytic cells

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16
Q

What does Eθ have to equal to be considered a spontaneous reaction?

A

Positive Value

17
Q

What equation calculates the overall cell potential?

A

The cell potential is the difference between the reduction potentials: Eocell=Eored−Eooxid

18
Q

What industrial situations use electrolytic cells?

A

Some examples of industrial situations in which electrolytic cells would be of use include metal plating and copper purifications.

19
Q

What is a galvanic cell?

A

A cell in which spontaneous oxidation- reduction reactions produce electrical energy

20
Q

What is an electrode?

A

A solid conductor of electricity

21
Q

What is an electrolyte?

A

A solution that contains positive ions (cations) and negative ions (anions)

22
Q

What is an external circuit in a Galvanic cell?

A

Wires that connect the anode to the cathode and allow the movement of electrons to occur

23
Q

What is electrolysis?

A

The process by which electrical energy is passed into a cell to cause a non- spontaneous reaction to occur

24
Q

What is oxidation?

A

Oxidation is the loss of electrons

25
Q

What is the difference between cell potential and standard cell potential?

A

The cell potential is the measure of the potential difference between two half cells in an electrochemical cell.

26
Q

What is the gain of electrons called?

A

Reduction

27
Q

What is the job of the salt bridge in a Galvanic cell?

A

It is a connection between the 2 half cells that allows the movement of charged ions

28
Q

What is the standard electrode potential of a half-cell a measure of?

A

This potential is a measure of the energy per unit charge which is available from the oxidation/reduction reactions to drive the reaction

29
Q

What occurs at the anode?

A

Oxidation (Loss of electrons) occurs at the anode

30
Q

What occurs at the cathode?

A

Reduction (gain of electrons) occurs at the cathode

31
Q

What type of a reaction occurs in a Galvanic cell?

A

A spontaneous REDOX reaction

32
Q

What type of chemical reaction occurs in a galvanic cell, Spontaneous, or non- spontaneous?

A

Spontaneous

33
Q

What type of electrochemical cell contains a salt bridge?

A

Galvanic cell

34
Q

What type of electrochemical cell uses energy from an external source?

A

Electrolytic cell

35
Q

What type of electrode is needed for a molten electrolytic cell?

A

The electrode must be an inert material; have a higher melting point then the molten solution

36
Q

What type of reaction occurs in electrolytic cells?

A

A forced non- spontaneous reaction.

37
Q

Why does a Galvanic cell need to be separated into two half cells?

A

A forced non- spontaneous reaction.

38
Q

Why does a Galvanic cell need to be separated into two half cells?

A

In order to utilise the current produced and start or stop the spontaenous reaction

39
Q

Why is molten electrolysis rarely seen/used?

A

It requires a large amount of energy to both run the cell as well as to keep the solution molten.

Chemistry (9 decks)

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