Using Chemical Reactions to Produce Electricity: Cells and Batteries

The video tutorial explains how cells and batteries produce electricity through chemical reactions. It covers the workings of a simple cell using zinc and copper in an electrolyte, highlighting the oxidation and reduction processes. The tutorial also discusses rechargeable cells, which reverse chemical reactions to restore potential difference, and batteries, which are multiple cells connected in series. Additionally, it explores hydrogen fuel cells, where hydrogen and oxygen react to produce water and electricity, emphasizing their potential as a sustainable energy source.

What is the role of zinc in a simple cell?

• It forms hydrogen gas.

• It gets oxidized and loses electrons.

• It acts as an electrolyte.

• It is the less reactive metal.

How does a rechargeable cell differ from a simple cell?

• It involves reversible chemical reactions.

• It cannot be recharged.

• It does not produce a potential difference.

• It uses only one type of metal.

What is a battery composed of?

• A single cell.

• Only zinc and copper.

• Multiple cells connected in series.

• A single metal and an electrolyte.

In a hydrogen fuel cell, what is the main product of the reaction between hydrogen and oxygen?

• Hydrochloric acid

• Methane

• Water

• Carbon dioxide

What is a significant environmental benefit of using hydrogen fuel cells?

• They produce carbon emissions.

• They use rare metals.

• They only produce water as a waste product.

• They require fossil fuels.