Electrochemical cells

Last updated: 10/02/2020

Edexcel A-Level Chemistry Redox II Electrochemical cells

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Question 1 of 18

1. Question
How is an electrochemical cell made?
- Connecting together two half cells
- Connecting together two solutions
- Connecting together two different elements
- Connecting together two different cells
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Question 2 of 18

2. Question
How are two half cells connected?
- Using a salt bridge and wire
- Using a voltmeter
- Using a wire
- Using a salt bridge
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Question 3 of 18

3. Question
What is a rechargeable cell?
- Provide electrical energy, cell reactions can be reversed whilst being recharged
- Provide electrical energy until the chemicals have reacted until the voltage fails
- Provides electrical energy from the sun
- Uses external supplies of fuel with an oxidant
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Question 4 of 18

4. Question
What is a non-rechargeable cell?
- Provide electrical energy until the chemicals have reacted until the voltage fails
- Provide electrical energy, cell reactions can be reversed whilst being recharged
- Provides electrical energy from the sun
- Uses external supplies of fuel with an oxidant
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Question 5 of 18

5. Question
What is the cell reaction?
- The difference in reduction and oxidation reactions taking place in each half cell
- The sum of the reduction and oxidation half reactions taking place
- The sum of the reduction and oxidation half reactions taking place in each half cell
- The difference in reduction and oxidation reactions taking place
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Question 6 of 18

6. Question
What is a fuel cell?
- Uses external supplies of fuel with an oxidant
- Provides electrical energy from the sun
- Provide electrical energy, cell reactions can be reversed whilst being recharged
- Provide electrical energy until the chemicals have reacted until the voltage fails
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Question 7 of 18

7. Question
How does a fuel cell work?
- Uses energy from the reaction of a fuel with oxygen
- Uses energy from the oxidation of oxygen
- Uses energy to fuel a reaction within a battery
- Uses electrical energy to react chemicals in the cell
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Question 8 of 18

8. Question
How can you calculate the standard cell potential?
- Standard electrode potential of the positive terminal – standard electrode potential of the negative terminal
- Standard electrode potential of the positive terminal x standard electrode potential of the negative terminal
- Standard electrode potential of the negative terminal – standard electrode potential of the positive terminal
- Standard electrode potential of the positive terminal + standard electrode potential of the negative terminal
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Question 9 of 18

9. Question
What is the symbol for the standard cell potential?
- $E_{cell}^ө$
- $E_c^ө$
- $E_{cl}^ө$
- $E_{CE}^ө$
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Question 10 of 18

10. Question
What happens to the electrode potential when there is a concentration change in a half cell?
- The electrode potential changes depending on the equilibrium
- The electrode potential does not change
- The electrode potential changes depending on which half cell concentration is changed
- The electrode potenial will increase
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Question 11 of 18

11. Question
What is the trend between the difference in standard electrode potential and the likelihood of a reaction?
- The larger the difference between standard electrode potentials, the more likely a reaction is to happen
- The larger the difference between standard electrode potentials, the less likely a reaction is to happen
- There is no relationship between the difference in standard electrode potential and the likelihood of a reaction
- The smaller the difference between standard electrode potentials, the more likely a reaction is to happen
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Question 12 of 18

12. Question
Which of the following is an example of a rechargeable cell?
- Nickel and cadmium
- Hydrogen rich cell
- Methanol
- Carbon battery
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Question 13 of 18

13. Question
Within a fuel cell, which hydrogen system provides the electrons?
- The more negative hydrogen system
- The less aqueous hydrogen system
- The more aqueous hydrogen system
- The more positive hydrogen system
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Question 14 of 18

14. Question
Within a fuel cell, which hydrogen system removes the electrons?
- The more positive hydrogen system
- The more aqueous hydrogen system
- The more negative hydrogen system
- The less aqueous hydrogen system
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Question 15 of 18

15. Question
What happens when constructing half equations at each electrode?
- Equilibrium is reversed
- Equilibrium stays still
- Equilibrium shifts to the left
- Equilibrium shifts to the right
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Question 16 of 18

16. Question
What is a drawback of using a lithium cell?
- It is toxic
- They get used up rapidly
- It is expensive
- Pollutes carbon dioxide into the air
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Question 17 of 18

17. Question
How is the difference in electrode potential measured?
- Using a voltmeter
- Using a cell
- Using a battery
- Using a fuel cell
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Question 18 of 18

18. Question
What is the minimum difference in standard electrode potential for a reaction to take place?
- 0.4 V
- 1.4 V
- -0.1 V
- 0 V
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