Electrode potentials Flashcards

1
Q

How is an electrochemical cell created

A

By joining 2 different half cells together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

With electrochemical cells, what is needed to join the 2 half cells together

A

A wire

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

In electrochemical cells what does the voltmeter measure

A

The potential difference between the 2 half cells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Do electrons flow from a more reactive metal to a less reactive metal, or from a less reactive metal to a more reactive metal

A

From a more reactive metal to a less reactive metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is observed when the half cell loses the electrons

A

The electrode becomes thinner

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What time of reaction is it when the half cell loses electrons and the electrode becomes thinner

A

Oxidation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What type of reaction occurs when the half cell accepts electrons and the electrode gets thicker

A

Reduction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the usual compound that creates a salt bridge

A

Potassium nitrate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the electrode potential measured in

A

Volts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What does the electrode potential tell us

A

How easily the half cell gives up electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

When writing electrochemical cell equations, in what form at the equations written

A

In reduced form, so electrons are always on the left hand side

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

When given the electrode potential values, what does the more negative value indicate( oxidation or reduction)

A

Oxidation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

When given the electrode potential values, what does the most positive value indicate (oxidation or reduction)

A

Reduction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What does SHE stand for

A

Standard hydrogen electrode

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the electrode potential of SHE

A

O volts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

When setting up a SHE, what are the conditions underwhich hydrogen enters the the system

A
  • 298 K
  • 100 kPa
17
Q

What are the conditions when comparing electrode potential values

A
  • Temp: 298 K
  • Pressure: 100 kPa
  • Concentrations of ions at 1 moldm^-3
18
Q

What does the SHE allow us to find

A

The standard electrode potential of other half cells

19
Q

When given a table of standard electrode values, what is the most powerful oxidising agent

A

The most positive standard electrode value

20
Q

When given 2 equations and the electrode potential, which reaction would go forward

A

The equation with the more positive electrode potential

21
Q

What does the electrode potential say

A

How much energy is released

22
Q

When drawing electrochemical cells what are the features that you must include

A
  • 2 half cells
  • Wire
  • Voltmeter
  • Salt bridge
  • 2 Electrodes
  • The electrodes must be under the water
23
Q

If the half cell is a metal, what is the electrode made of

A

The same metal
e.g. Fe2+ +2e- -> Fe
use a Fe electrode

24
Q

If neither half cells include a metal, what electrode should you use

A
  • An inert metal like platinum
  • Or graphite
25
What is the role of a salt bridge
Balances charges
26
Does the salt bridge carry ions or electrons
Ions
27
How do you assign the positive or negative charge to the electrode
The electrode that receives the electrons is the positive electrode
28
When drawing an electrochemical cell, what should you draw on the wire and on the salt bridge
The direction the electrons/ ions flow
29
What is the electrode that is used when using a hydrogen half cell
Platinum
30
How do you use a hydrogen half cell
Use a platinum electrode and bubbles hydrogen gas over it using a glass tube
31
What is the standard electrode potential of a half cell
The voltage measured in a cell in which that half cell is connected to a standard hydrogen electrode, under standard conditions
32
What 2 gases are in fuel cells
- Hydrogen - Oxygen
33
In a hydrogen fuel cell, what is oxidised the hydrogen or the oxygen
Hydrogen
34
In acidic conditions, what is the equation of a hydrogen fuel cell
Oxygen + 2Hydrogen -> 2 Water
35
In alkali conditions, what is the equation of a hydrogen fuel cell
Oxygen + 2 Hydrogen -> 2 Water
36
What are the main issues around hydrogen fuel cells
- Explosive - Compressed into a small battery - Producing the hydrogen may produce carbon dioxide, so no better than other batteries