O Levels Chemistry (5070)•5070/11/M/J/21
Explanation
Le Chatelier's Principle and Reaction Kinetics
Steps:
- Identify changes: Volume halved while pressure constant requires temperature adjustment; explicit increase to 500°C.
- Apply ideal gas law: Constant P with halved V and raised T decreases concentration (c = P/RT).
- Assess rate: Higher temperature always increases reaction rate via Arrhenius equation.
- Determine shift: Decreased concentration favors side with more particles; without reaction stoichiometry, direction unclear.
Not enough information to determine equilibrium shift or confirm option A.
Why A is correct: Insufficient details on reaction (e.g., Δn, endothermic/exothermic) prevent validation.
Why the others are wrong:
- B: Rate increases with temperature, not decreases.
- C: Shift direction unknown without Δn.
- D: Both rate and shift unconfirmed.
Final answer: Not enough information.
Topic: Reversible reactions and equilibrium
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