Instant Crystals

The video tutorial explains the process of crystallization, focusing on how sodium ethanoate can form crystals rapidly. It begins with an introduction to crystal formation, followed by a step-by-step guide to preparing a supersaturated solution. The demonstration shows how adding a small amount of solid sodium ethanoate to the solution causes rapid crystallization, forming a stalagmite structure. The tutorial also covers the concept of supersaturation and its practical applications, such as in hand warmers, where a disturbance in the solution leads to an exothermic reaction that generates heat.

What is the purpose of using a conical flask in the crystallization experiment?

• To store the final crystals

• To act as a heat source

• To dissolve sodium ethanoate in water

• To measure the temperature of the solution

What happens to the sodium ethanoate crystals when water is added?

• They immediately crystallize

• They remain unchanged

• They dissolve completely

• They begin to dissolve but the solution becomes saturated

Why is it important to cool the solution slowly after heating?

• To prevent the solution from evaporating

• To speed up the crystallization process

• To ensure the solution remains clear

• To avoid disturbing the supersaturated state

What role does the solid sodium ethanoate play in the crystallization process?

• It acts as a solvent

• It serves as a nucleation site

• It prevents crystallization

• It dissolves in the solution

How does the crystallization process create a stalagmite structure?

• By cooling the solution quickly

• By heating the solution rapidly

• By stacking crystals on top of each other

• By dissolving the crystals in water

What triggers the crystallization in hand warmers?

• Adding more water

• Heating the solution

• Snapping a small piece of metal

• Cooling the solution

What type of reaction occurs when the hand warmer crystallizes?

• Endothermic reaction

• Decomposition reaction

• Exothermic reaction

• Neutralization reaction