Primary galvanic cells and fuel cells as sources of energy
Redox reactions involve simultaneous processes of oxidation and reduction, where electrons are transferred between chemical species, resulting in changes in their oxidation states. These reactions are fundamental to many chemical processes, such as combustion reactions, which convert chemical energy into heat, and Galvanic and fuel cells, which produce electrical energy.
We use the electrochemical series to predict whether a redox reaction will occur spontaneously and to calculate maximum cell voltage under standard conditions. Faraday’s Laws allow us to quantify relationships between current, time and the amounts of reactants or products in electrochemical reactions.
In our modern, energy-reliant world, redox chemistry underpins critical technologies like batteries and fuel cells, and provides us with options for sustainable energy solutions.
This resource revises primary galvanic cells and fuel cells as sources of energy and within this topic there are 3 key concepts
To determine if this resource will benefit you, start by answering the following questions.
- How does the change in oxidation numbers help to identify the oxidising and reducing agents, as well as oxidation and reduction half equations?
- How are half redox equations and overall redox equations balanced?
- How are the electrochemical series used to predict redox reaction outcomes and determine the maximum cell voltage under standard conditions?
- What are the key design features of non-rechargeable galvanic cells, and how do these features enable the conversion of chemical energy to electrical energy?
- How can Faraday’s Laws and stoichiometry be applied to calculate reactants, products, current, or time in electrochemical cells?
The answers to these questions are provided on the following pages. Use this resource to refresh your memory, reinforce your understanding of these concepts, and prepare more effectively for university-level learning.