고등 수준: 평형 교란에 대한 반응을 예측하기
도입됨| English | 의미 |
|---|---|
| Le Chatelier’s Principle/lə ˈtʃeɪtlɪəz ˈprɪnsɪpl/ | 르 샤틀리에 원리 |
| equilibrium shift/ˌiːkwɪˈlɪbrɪəm ʃɪft/ | 평형 이동 |
What would explain this observation?
- Higher Tier: An equilibrium mixture responds when a condition changes. Its response opposes the disturbance, but does not necessarily restore the original amounts exactly.
- Start with a prediction. State the quantities or features you would compare, then decide what evidence could distinguish two explanations.
Build the model
- Equilibrium amounts depend on reaction conditions. Le Chatelier’s Principle 勒沙特列原理 states that when a system at equilibrium is disturbed, it responds to counteract the change. After a change of concentration, temperature or reacting-gas pressure, the system adjusts until forward and reverse rates are equal again. Predict qualitatively which direction is favoured using the equation and the changed condition. This entire source section is Higher-only.
- Le Chatelier’s Principle: An equilibrium system responds to a disturbance in a direction that counteracts it; equilibrium shift 平衡移动: A net composition adjustment toward a new equilibrium after conditions change.
교란 후 새로운 평형을 설명하는 문장은?
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교란 이후 시스템은 정방향과 역방향 속도가 다시 일치할 때까지 이동합니다 - 그 평등함이 새로운 평형을 정의합니다. 선호되는 방향만 독립적으로 진행되지 않으며, 새로운 농도는 일반적으로 원래와 다릅니다.
각 전문 용어에 대한 정확한 의미를 매칭하시오.
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정의를 사용하여 유사한 양과 과정을 구분하시오.
Choose evidence that can test it
- Begin with the system already at equilibrium, identify one imposed change and select the appropriate response rule. Increased reactant concentration favours its consumption; removing product favours forming more. Warming favours the endothermic direction. Compression of a gaseous equilibrium favours the side with fewer gas molecules. These are composition responses, not the same as saying every faster reaction makes a larger final yield.
- Use supplied equations, forward energy direction, states and before/after data. Mark a shift arrow as net adjustment toward a new equilibrium, not cessation of the other reaction. Keep other conditions specified. A suitable catalyst increases both rates and reduces time to equilibrium without shifting the final equilibrium composition at fixed conditions. No equilibrium-constant expression or numerical constant calculation is required by this GCSE section.
이 경우 조사 또는 모델이 더 타당하게 만들 수 있는 두 가지 습관은 무엇인가?
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조건과 가정을 명시하면 다른 사람이 정확히 작업을 재현할 수 있으며, 근거 증거를 기록하면 결론을 검증할 수 있습니다. 반대되는 결과를 숨기는 것은 잘못된 결론을 반박할 수 있는 증거를 제거하는 것이며, 한 번의 측정으로는 더 넓은 주장을 입증할 수 없습니다.
Work from known quantities
- State the known values and their units. Choose the relation because its assumptions fit this case, then rearrange before substitution.
- Known: a supplied one-to-one mixture initially contains 40 A and 60 B particles at equilibrium. After an imposed change and re-equilibration it contains 30 A and 70 B. Net B increase is ten, so the observed response favoured products. Total remains 100 in this stated closed conversion model. These data show a direction of shift but alone do not identify which condition was changed.
A supplied mixture changes from 55 to 68 product particles after re-equilibration. Find the product-count increase. Use the same sequence: known quantities → model → relation → substitution → unit and interpretation.
공급된 혼합물이 재평형화 후 생성물 입자를 55에서 68으로 바꾼다. 생성물 수의 증가분을 구하시오.
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결과는 13 입자입니다. 주어진 조건: 생성물 개수가 55 から 68 입자로 변화함. 증가량 = 68 - 55 = 13 입자. 평형은 생성물을 선호하게 이동했으나, 교란은 완전히 상쇄되지 않고 부분적으로만 반발됨.
Check the conclusion and its limits
- Do not describe counteracting as entirely cancelling the original disturbance. A catalyst does not count as a concentration addition of reactant. A shift toward products does not mean all reactants are consumed, and equal rates at the new equilibrium do not require the old mixture ratio. Different perturbations can produce the same direction of observed composition change.
- Return to the original observation. Explain what the result supports, which conditions it assumes, and one way to test a competing explanation.
Counteracting a disturbance always restores every original concentration exactly. This claim is false: The system counteracts the disturbance only PARTIALLY: it moves in the opposing direction but settles at new concentrations. The original mixture is not restored - a new equilibrium is established instead.
Higher Tier: predict the response to an equilibrium disturbance: Begin with the system already at equilibrium, identify one imposed change and select the appropriate response rule. Increased reactant concentration favours its consumption; removing product favours forming more. Warming favours the endothermic direction. Compression of a gaseous equilibrium favours the side with fewer gas molecules. These are composition responses, not the same as saying every faster reaction makes a larger final yield.
교란에 대항하는 반응은 항상 모든 원래 농도를 정확히 복원합니다.
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시스템은 교란에 대해 '부분적으로'만 대응합니다: 반대 방향으로 이동하지만 새로운 농도에서 정착됩니다. 원래 혼합물은 복원되지 않으며 대신 새로운 평형이 수립됩니다.
평형계는 교란에 대해 이를 상쇄하는 방향으로 반응합니다: 이 기술 용어를 적으십시오.
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르 샤틀리에 원리는 평형계가 교란에 대해 이를 상쇄하는 방향으로 반응함을 의미합니다.