반응 프로파일: 활성화 장벽과 전체 에너지 변화를 구분함
도입됨| English | 의미 |
|---|---|
| activation energy/ˌæktɪˈveɪʃn ˈenədʒi/ | 활성화 에너지 |
| reaction profile/rɪˈækʃn ˈprəʊfaɪl/ | 반응 에너지 도표 |
What would explain this observation?
- An exothermic reaction may still need a spark to start. Releasing energy overall does not remove the initial energy barrier that reacting particles must overcome.
- Start with a prediction. State the quantities or features you would compare, then decide what evidence could distinguish two explanations.
Build the model
- Reactions occur when particles collide with sufficient energy. Activation energy 活化能 is the minimum energy particles must have for the reaction to occur. A reaction profile 反应能量图 plots energy vertically against reaction progress horizontally. The reactant level leads up to a curved peak, then down to the product level. The activation-energy arrow runs from the reactant level to the peak; it is not measured from the graph’s arbitrary zero.
- activation energy: The minimum energy that particles must have for a reaction to occur; reaction profile: A diagram showing energy levels as a reaction progresses.
프로파일에서 생성물이 반응물보다 위에 있습니다. 이것이 나타내는 것은 무엇인가?
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생성물이 반응물 위에 그려지면 전체적으로 에너지를 얻었음을 의미하며, 이는 흡열 반응입니다. Activation barrier(활성화 장벽)인 봉우리는 여전히 존재하며, 흡열 프로파일에도 반드시 이 장벽이 있습니다.
각 전문 용어에 대한 정확한 의미를 매칭하시오.
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정의를 사용하여 유사한 양과 과정을 구분하시오.
Choose evidence that can test it
- In an exothermic profile products lie below reactants, showing an overall energy decrease of the reacting chemicals and transfer to surroundings. In an endothermic profile products lie above reactants, showing energy taken from surroundings. Both profiles can have an activation barrier. The vertical difference between reactants and products is the overall change, distinct from the larger climb to the peak. Horizontal distance is not elapsed time or a measured reaction rate.
- Draw axes first, mark clearly different reactant and product levels, then join them with a smooth curve rising above both. Label reactants, products and activation energy. Add a separate vertical arrow for the overall energy change. Compare the two diagrams using level differences, not the apparent length of the curve. Use relative energy units if numbers are supplied; they illustrate a model rather than requiring calorimetry.
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 relative-energy model has reactants at 30, peak at 85 and products at 10 units. Activation energy is 85−30=55 units; the reacting chemicals decrease by 30−10=20 units, so it is exothermic. If products instead lie at 50 with the same reactants and peak, the increase is 20 units and the reaction is endothermic. The initial barrier remains 55 units.
Relative reactant level is 25 and peak level is 90. Find the activation-energy difference. Use the same sequence: known quantities → model → relation → substitution → unit and interpretation.
상대 반응물 수준은 25이고, 최고점 수준은 90입니다. 활성화 에너지 차이를 구하십시오.
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결과는 65 상대 단위입니다.已知: 반응물 수준 25; 최고점 수준 90. 활성화 에너지 = 90 - 25 = 65 상대 단위. 장벽은 생성물이 아닌 반응물에서 최고점까지 측정됩니다.
Check the conclusion and its limits
- A peak is not an intermediate product that must be collected. Do not label reaction progress as time, equate activation energy to overall energy change or assume exothermic reactions always occur rapidly at room temperature. The source requires qualitative profiles; numerical relative levels are a way to practise reading their geometry.
- Return to the original observation. Explain what the result supports, which conditions it assumes, and one way to test a competing explanation.
Every exothermic reaction has zero activation energy. This claim is false: Every reaction needs enough collision energy to start breaking bonds - the activation energy. Exothermic describes the overall change from reactants to products; it says nothing about the size of the initial barrier.
Reaction profiles: distinguish the barrier from the overall change: In an exothermic profile products lie below reactants, showing an overall energy decrease of the reacting chemicals and transfer to surroundings. In an endothermic profile products lie above reactants, showing energy taken from surroundings. Both profiles can have an activation barrier. The vertical difference between reactants and products is the overall change, distinct from the larger climb to the peak. Horizontal distance is not elapsed time or a measured reaction rate.
모든 발열 반응은 활성화 에너지가 0입니다.
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모든 반응은 결합을 끊기 시작하기 위해 충분한 충돌 에너지를 필요로 하며 이것이 활성화 에너지입니다. 발열성은 반응물에서 생성물로 가는 전체 변화를 설명할 뿐 초기 장벽의 크기에 대해서는 아무것도 말하지 않습니다.
반응이 일어나기 위해 입자가 가져야 할 최소 에너지: 기술적 용어를 쓰십시오.
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활성화 에너지(activation energy)는 반응이 일어나기 위해 입자가 가져야 할 최소 에너지를 의미합니다.