Dry Ice and Magnesium

The video explores how carbon dioxide, typically used to extinguish flames, can instead fuel combustion under certain conditions. An experiment is conducted using magnesium and dry ice to demonstrate this phenomenon. The magnesium burns in a redox reaction, stripping oxygen from carbon dioxide, resulting in magnesium oxide and elemental carbon. The video highlights the importance of understanding chemical reactions and the limitations of carbon dioxide extinguishers on metal fires.

What is the primary role of carbon dioxide in extinguishing flames?

• To add moisture to the air

• To increase the temperature

• To cut off the supply of oxygen

• To provide fuel for the fire

What protective gear is necessary when handling dry ice and magnesium?

• Sunglasses and a hat

• Sunglasses and protective gloves

• A lab coat and boots

• A mask and earplugs

What is the initial reaction when magnesium is ignited?

• It reacts with carbon dioxide to form carbon monoxide

• It reacts with hydrogen to form magnesium hydride

• It reacts with nitrogen to form magnesium nitride

• It reacts with oxygen to form magnesium oxide

What type of reaction occurs when magnesium strips oxygen from carbon dioxide?

• A reduction reaction

• A synthesis reaction

• A decomposition reaction

• A neutralization reaction

What are the visible products of the reaction between magnesium and carbon dioxide?

• Magnesium carbonate and water

• Magnesium oxide and elemental carbon

• Carbon monoxide and magnesium nitride

• Magnesium chloride and carbon dioxide

Why can't carbon dioxide extinguishers be used on metal fires?

• They are not environmentally friendly

• They are ineffective due to the redox reaction

• They increase the fire's intensity

• They are too expensive

What is the overall type of reaction observed in the experiment?

• An acid-base reaction

• A precipitation reaction

• A combustion reaction

• A redox reaction