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The Cool Reaction Thermodynamics Chemistry Demonstration Kit shows that endothermic reactions can be just as exciting as exothermic reactions. One example is when the solids barium hydroxide and ammonium thiocyanate are mixed together in a beaker.

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Many reactions produce heat. In fact, when students think of chemical reactions, heat production is often expected. However, endothermic reactions—reactions that consume heat—can be just as exciting. One of the most striking examples of this is when the solids barium hydroxide and ammonium thiocyanate are mixed together in a beaker. Teacher Demonstration Notes included. 

Concepts: Endothermic reactions.
Time Required: 20 minutes .
Note: A thermometer is required and available separately.

Correlation to Next Generation Science Standards (NGSS)

Science & Engineering Practices

Developing and using models
Analyzing and interpreting data
Engaging in argument from evidence

Disciplinary Core Ideas

MS-PS1.B: Chemical Reactions
MS-PS3.B: Conservation of Energy and Energy Transfer
MS-PS3.D: Energy in Chemical Processes and Everyday Life
HS-PS1.B: Chemical Reactions
HS-PS3.B: Conservation of Energy and Energy Transfer
HS-PS3.D: Energy in Chemical Processes

Crosscutting Concepts

Cause and effect
Systems and system models
Energy and matter

Performance Expectations

MS-PS1-2. Analyze and interpret data on the properties of substances before and after the substances interact to determine if a chemical reaction has occurred.
HS-PS1-5. Apply scientific principles and evidence to provide an explanation about the effects of changing the temperature or concentration of the reacting particles on the rate at which a reaction occurs.
HS-PS1-7. Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction.