Labs / Chemistry
Energy Diagram
Every reaction has to climb an energy hill before it can roll downhill to products. Slide the enthalpy and activation energy to reshape the curve, then flip in a catalyst and watch it carve out an easier path over the same reaction.
ΔH -160 kJ/molEa 90 kJ/molExothermicE 180 kJ/molprogress 0%
What to try
- When products sit lower than reactants, where does the released energy come from — and is that exothermic or endothermic?
- Turn on the catalyst. Does it change ΔH, or only the height of the barrier the marker has to cross?
- Raise the barrier while keeping ΔH fixed. Why does the marker crawl so slowly over the top?
- Can you build a reaction that gives out heat but still has a huge activation energy — like a log that won't light without a match?
- Compare the climb from reactants versus from products. Which direction faces the taller hill, and what does that say about the reverse reaction?