Mississippi Science CHE.10.2
The Standard
- CHE.10
- Enrichment: Students will understand that energy is exchanged or transformed in all chemical reactions.
Enrichment: Classify chemical reactions and phase changes as exothermic or endothermic based on enthalpy values. Use a graphical representation to illustrate the energy changes involved.
2026 Mississippi College- and Career-Readiness Standards for Science · Thermochemistry (Enrichment)
Teacher's field guide
What This Standard Means
What Students Need to Do
- Students use the sign of an enthalpy change to tell whether a reaction or phase change absorbs or releases heat. They draw an energy diagram showing the starting and ending energy levels.
What Mastery Looks Like
- Given a positive or negative enthalpy change, students correctly name the process as endothermic or exothermic. Their diagram puts the ending state at the right energy level and labels the change with the correct sign.
Common Misconceptions
- Students may think a negative enthalpy change means the system gains heat. They may put products higher on an exothermic diagram or say melting ice releases heat because it feels cold.
How to Assess It
- Exit ticket: A reaction has ΔH = −80 kJ, and melting ice has ΔH = +6 kJ. Classify both, then draw a labeled energy diagram for the reaction.
Lesson moves
Ways to Teach It
Measure water temperature before and after adding ice, then use a +6 kJ/mol card to sketch an energy diagram for melting.
Show two diagrams with different ending energy levels and ask, "Which process absorbs heat, and how can you tell?"
Sort cards for melting ice (+6 kJ/mol), freezing water (−6 kJ/mol), and methane combustion (−890 kJ/mol), then sketch matching diagrams.
Compare ice melting in a drink with water freezing in a freezer, and draw arrows showing where heat goes in each case.
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Printable CHE.10.2 Worksheet
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