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Chemical cells and fuel cells (chemistry only)
This chemistry-only topic links electrochemical reactions, electrodes, electrolytes and oxidation to electricity generation in simple cells, batteries and hydrogen fuel cells.
23
Objectives
115
Flashcards
115
Questions
90 min
Study time
AQAGCSEChemistryEnergy changes
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Syllabus checklist
What you need to know
23 objective pages available
Cells and batteries12 objectives
- (chemistry only) Describe that cells contain chemicals that react to produce electricity.
- (chemistry only) Explain that the voltage produced by a cell depends on factors including electrode type and electrolyte.
- (chemistry only) Describe a simple cell as two different metals in contact with an electrolyte.
- (chemistry only) Explain why two different electrodes are needed in a simple chemical cell.
- (chemistry only) Describe batteries as two or more cells connected together in series.
- (chemistry only) Explain why connecting cells in series provides a greater voltage.
- (chemistry only) Describe that reactions in non-rechargeable cells stop when one reactant is used up.
- (chemistry only) Identify alkaline batteries as non-rechargeable.
- (chemistry only) Explain that rechargeable cells and batteries can be recharged because their chemical reactions are reversed by an external electrical current.
- (chemistry only) Interpret data for relative reactivity of different metals in cells.
- (chemistry only) Evaluate the use of cells from information about voltage, electrode materials, electrolyte and rechargeability.
- (chemistry only) Describe safe and careful use of liquids when investigating cells. (AT 6)
Fuel cells11 objectives
- (chemistry only) Describe fuel cells as being supplied by an external source of fuel and oxygen or air.
- (chemistry only) State that hydrogen can be used as the fuel in a fuel cell.
- (chemistry only) Explain that the fuel is oxidised electrochemically within a fuel cell.
- (chemistry only) Explain that a fuel cell produces a potential difference.
- (chemistry only) State that the overall reaction in a hydrogen fuel cell involves oxidation of hydrogen to produce water.
- (chemistry only) Explain why hydrogen fuel cells can be considered as an alternative to rechargeable cells and batteries.
- (chemistry only) Evaluate advantages and disadvantages of hydrogen fuel cells compared with rechargeable cells and batteries.
- (chemistry only) Compare fuel supply, products, rechargeability and operating use for fuel cells and rechargeable batteries.
- (chemistry only) (HT only) Write the half equation for the hydrogen electrode reaction in a hydrogen fuel cell when formulae and charges are supplied.
- (chemistry only) (HT only) Write the half equation for the oxygen electrode reaction in a hydrogen fuel cell when formulae and charges are supplied.
- (chemistry only) (HT only) Link hydrogen fuel cell half equations to the overall production of water.
Key terms
cellelectrolyteVoltageElectrodesimple cellelectrodechemical cellbatteryseries connectionvoltageNon‑rechargeable cellReactant depletion
Exam tips
- Understand Cell Chemistry: Explain clearly: Explain remember that cells contain chemicals that react to produce electricity. Focus on the types of chemicals involved and their roles in the reaction. Link your answer to Cells and batteries in Chemical cells and fuel cells (chemistry only); for bond-energy work, separate bonds broken from bonds formed and include the sign and unit.
- Understand Factors Affecting Voltage: Explain review how different electrode materials and electrolytes influence the voltage of a cell. Link your answer to Cells and batteries in Chemical cells and fuel cells (chemistry only); for bond-energy work, separate bonds broken from bonds formed and include the sign and unit.
Common mistakes
- Misunderstanding Cell Composition: Emphasize that cells consist of two different metals and an electrolyte, which is crucial for the chemical reactions that generate electricity.
- Misattributing voltage to only the electrolyte: Explain that the cell voltage depends on the difference in electrode potentials of the two metals and the nature of the electrolyte, which affects ion mobility and reaction rates but does not alone set the voltage
Practice preview
- What is the energy-transfer idea behind a chemical cell producing electricity?
- Why will a non-rechargeable cell eventually stop producing electricity?
- For Cells and batteries, which answer best supports this AQA GCSE Chemistry Unit 4.5 objective: (chemistry only) Describe that cells contain chemicals that react to produce electricity?
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