Electrode potentials, cells and the Nernst equation – Primrose Kitten

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Electrode potentials, cells and the Nernst equation

Last updated: 14/03/2020

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Question 1 of 22

1. Question
What is the definition of the electrochemical series?
- Listing half-cells in order of their standard electrode potentials
- Listing chemicals in terms of their voltage
- Listing half-cells in terms of their voltage
- Listing chemicals in order of their standard electrode potentials
Question 2 of 22

2. Question
What is the definition of a half cell?
- Holds an element in two oxidation states
- Conditions two redox reactions
- One half of a redox reaction
- A cell within a battery
Question 3 of 22

3. Question
What is the definition of a standard electrode potential of a half-cell?
- The voltage of a half-cell compared with a standard hydrogen half-cell
- The voltage of a half-cell compared with a standard half-cell
- The voltage of a half-cell compared with a standard carbon half-cell
- The voltage of a half-cell compared with a standard platinum half-cell
Question 4 of 22

4. Question
What is the symbol for the standard electrode potential of a half-cell?
- $E^ө$
- $S^ө$
- $P^ө$
- $T^ө$
Question 5 of 22

5. Question
What is needed to calculate the electrode potential change?
- Concentration change
- Volume change
- Ideal gas
- Pressure change
Question 6 of 22

6. Question
How can the standard electrode potential of a half-cell be determined?
- Measure against a hydrogen half-cell
- Measure with a voltmeter
- Measure against hydrogen
- Measure against platinum
Question 7 of 22

7. Question
How are salt bridges made?
- Using filter paper soaked in an aqueous solution
- Using filter paper coated in sodium hydroxide
- Using a wire in solution
- Using a metal rod
Question 8 of 22

8. Question
When measuring the standard electrode potential, what is the purpose of a salt bridge?
- Connects the two solutions and allows the ion carrying charge to be transferred
- Enables the redox reactions
- Starts the reaction
- Carries the electron carrying charge
Question 9 of 22

9. Question
When measuring the standard electrode potential, what is the purpose of the wire?
- Carries the electron carrying charge
- Connecting two solutions
- Enables the redox reactions
- Transfers ion charges
Question 10 of 22

10. Question
What is the purpose of the platinum electrode?
- To be in contact with the hydrogen ions and hydrogen, transferring electrons
- To act as a battery
- To connect both solutions
- To carry an electric current
Question 11 of 22

11. Question
What is the surface of the platinum electrode coated with?
- Platinum black
- Electricity
- Water
- Sodium hydroxide
Question 12 of 22

12. Question
What is needed to allow a hydrogen half-cell to work?
- Platinum electrode
- Aqueous solution
- Copper electrode
- Carbon electrode
Question 13 of 22

13. Question
Why does a hydrogen half-cell not work alone?
- There is no solid to act as an electrode
- No current can be carried
- The gas will evaporate
- It is not reactive enough
Question 14 of 22

14. Question
What does a metal ion/metal ion half-cell contain?
- Ions of two different metals
- Gaseous solutions of two metals
- Solution of two metals
- Ions of the same metals in different oxidation states
Question 15 of 22

15. Question
Which direction is preferred when a half-cell has a positive electrode potential value?
- Right hand side
- Left hand side
- Neither side
- It will depend on the elements involved
Question 16 of 22

16. Question
Which direction is preferred when a half-cell has a negative electrode potential value?
- Left hand side
- Right hand side
- Neither side
- It will depend on the elements involved
Question 17 of 22

17. Question
What is the voltage of a hydrogen half-cell?
- 0 V
- 0.34 V
- -0.2 V
- 0.5 V
Question 18 of 22

18. Question
Write the equation for a hydrogen half-cell.
- $2H^+(aq) + 2e^- -> H_2(g)$
- $H^+(aq) + e^- -> H_2(g)$
- $2H^+(aq) + 2e^- -> 2H_2(g)$
- $2H^+(l) + 2e^- -> H_2(g)$
Question 19 of 22

19. Question
What equation is used to calculate electrode potential changes?
- Nernst equation
- Avogadro equation
- Ideal gas equation
- Enthalpy change
Question 20 of 22

20. Question
What is the Nernst equation?
- Eo + (0.059/z) log [oxidised species] / [reduced species]
- Eo + (0.059/z) log [oxidised species] x [reduced species]
- Eo + (0.059/z) [oxidised species] / [reduced species]
- Eo + (0.059) log [oxidised species] / [reduced species]
Question 21 of 22

21. Question
What type of species is needed for the Nernst equation?
- Oxidised
- Acidic
- Neutral
- Basic
Question 22 of 22

22. Question
What type of species is needed for the Nernst equation?
- Reduced
- Acidic
- Neutral
- Basic

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