Redox reactions, which are short for reduction-oxidation reactions, are important in many things we see every day. Let’s look at some common examples:

1. Rusting of Iron:

   • This happens when iron (Fe) meets oxygen (O₂) and water (H₂O).
   • The chemical reaction can be written like this: $4Fe + 3O_2 + 6H_2O \rightarrow 4Fe(OH)_3$
   • Each year, about 1.5 billion tons of iron rust away because of this process.

2. Combustion:

   • This is when fuels like natural gas (methane) burn.
   • Here’s a simple reaction to show this: $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$
   • In the U.S., around 70% of our electricity comes from burning fossil fuels.

3. Photosynthesis:

   • This is how plants turn sunlight into energy.
   • The overall reaction looks like this: $6CO_2 + 6H_2O + light \rightarrow C_6H_{12}O_6 + 6O_2$
   • Plants produce about 280 billion tons of glucose every year through this process.

4. Batteries:

   • Batteries use redox reactions to create electrical energy.
   • For example, in alkaline batteries, one reaction looks like this: $Zn + 2MnO_2 \rightarrow ZnO + Mn_2O_3$
   • The battery market is expected to grow to $120 billion by 2025, showing how important redox reactions are in our technology.

Redox reactions play a key role in many everyday processes, from rusting to powering our devices!