Electrode Potentials and Electrochemical Cells

Question 1

Based on electrode potentials, what is the strongest oxidising or weakest reducing agent?

Answer 1

The ion with the most positive value

Question 2

Based on electrode potentials, what is the weakest oxidising or strongest reducing agent?

Answer 2

The ion with the most negative electrode potential

Question 3

What are the standard conditions for electrode potentials?

Answer 3

298k
100kPa (only for gas!!!)
1moldm^3

Question 4

Why is hydrogen fuel not carbon neutral?

Answer 4

Co2 is released as fossil fuel is burned to generate hydrogen

Question 5

Suggest a possible salt for a salt bridge

Answer 5

Potassium nitrate kNO3 solution unless half cells have either potassium or nitrogen
Or potassium chloride

Question 6

Which way do electrons flow in an electrochemical cell?

Answer 6

To the reduced ion, away from the oxidised ion

Question 7

What type of reaction goes on in a cell?

Answer 7

Redox

Question 8

What electrode should be used for Fe3+?

Answer 8

Platinum bc it’s inert and allows for the flow of electrons

Graphite can be used as an alternative

Question 9

Why are electrode potentials always written as a reduction reaction?

Answer 9

Because they are being compared to the standard hydrogen electrode

Question 10

Which half cell will reduce which?

Answer 10

The more positive the electrode will oxidise the more negative electrode

Question 11

Which half cell will be reduced?

Answer 11

The more positive half cell

Question 12

How do you work out the electrode potentials of cell?

Answer 12

RHS-LHS
Reduced-oxidised
More positive-more negative

Question 13

What is the value of the standard hydrogen electrode?

Answer 13

0.00V

Question 14

EMPIRIO

Answer 14

E
Most 
Positive 
Is 
Reduced
It 
Oxidises

Question 15

What is the purpose of a salt bridge?

Answer 15

To complete the circuit

To allow ions in the ionic substance in the salt bridge to move through the salt brigdhe