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MDCAT Worksheet

⚖ Equilibrium & Le Chatelier's Principle

Chapter: Chemistry · Level ★★★ · Time: 25 min
SCORE___ / 20
NameClassDate
After this worksheet you can
Define chemical equilibriumInterpret KcApply Le Chatelier's principleExplain the Haber process conditions
📚 Quick Recap

🎯 What you'll practice: Equilibrium basics, Kc, Le Chatelier shifts, and the Haber process as a worked example.

🧠 Section A · Concept Check ● BEGINNER 4 × 1 = 4

1At equilibrium, forward and reverse rates are:
2If Kc > 1, the reaction favours:
3A catalyst affects equilibrium position by:
4Haber process catalyst:

🧮 Section B · Problem Solving ● INTERMEDIATE 2 + 3×3 = 11

5Increasing pressure shifts equilibrium toward the side with gas moles.
6The Haber process operates at approximately atm.
7Write the balanced equation for the Haber process.
8What happens to equilibrium if you add more product to the mixture?
9Why does the Haber process use ~400°C rather than a much higher temperature?

🚀 Section C · Challenge ● CHALLENGE 5

10The Haber reaction N₂ + 3H₂ ⇌ 2NH₃ is exothermic in the forward direction. Explain, using Le Chatelier's principle, why increasing temperature actually reduces NH₃ yield even though it speeds up the reaction.
💭 Reflection — the most useful thing I learned:
A ___/4   B ___/11   C ___/5   Total ___/20 Teacher's Signature Parent's Signature
✂ answer key — fold or cut before handing out

1-A   2-B   3-C   4-B  |  5 = fewer   6 = 200   7 = N2 + 3H2 ⇌ 2NH3   8 = equilibrium shifts left, back toward reactants, to partly consume the added product   9 = because a much higher temperature would shift equilibrium further away from NH3 (the exothermic forward direction), even though it would make the reaction faster — 400°C is chosen as a compromise between reasonable reaction rate and acceptable yield  |  10 = Because the forward reaction is exothermic, raising temperature shifts equilibrium toward the endothermic (reverse) direction to absorb the extra heat, converting some NH3 back into N2 and H2 — so even though the higher temperature makes the system reach equilibrium faster, the equilibrium position itself moves toward less NH3, which is why industrial Haber plants use a moderate 400°C rather than a very high temperature.

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