Name: arrhenius equation in reaction speed
Uploaded: 2023-04-30T18:28:32.000Z
Duration: 2 min 28 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-5

effect-of-temperature-change-on-reaction-rate

Effect of Temperature Change on Reaction Rate

반응의 속도 법은 반응 농도와 반응 비율 사이의 관계를 일정한 비율로 정의합니다.
속도 상수는 Arrhenius 방정식을 통해 반응 분자의 충돌, 방향 및 활성화 에너지와 관련된 온도 와 운동 매개 변수 사이의 관계를 설명합니다. 'A는아레니우스 인자 또는 주파수 인자라고 하는 상수입니다. 'e'는두더지당 주들, 가스 상수 및 켈빈의 온도로 측정된 활성화 에너지를 통합하는 기하급수적 인요인입니다.
파라미터의 온도 의존성은 반응 분자가 화학 반응을 시작하기 위해 올바른 방향으로 충분한 에너지와 충돌해야 한다는 것을 나타내는 충돌 모델과 설명될 수 있다.
주파수 계수는 충돌 빈도와 방향 계수의 두 구성 요소를 구성합니다. 충돌 빈도는 단위 시간당 분자 충돌 횟수이며 방향 계수는 유리한 방향으로 충돌할 확률을 설명합니다.
그럼에도 불구하고 충돌의 극히 일부만 반응으로 이어집니다. 이는 반응 분자가 활성화 에너지라고 하는 에너지 장벽을 극복하여 제품으로 전환해야 하기 때문입니다.
충분한 운동 에너지와 충돌하는 분자만이 전환 상태 또는 활성화된 복합체라고 하는 고에너지 중간체로 변환하기 위해 결합을 구부리거나, 스트레칭하거나, 분해할 수 있는 충분한 잠재적 에너지를 갖게 됩니다. 단명하고 불안정한 활성화 된 복합체는 에너지를 잃어 안정적인 제품을 형성하며 총 에너지가 반응자보다 낮습니다.
Arrhenius 방정식의 지수 요인은 성공적인 충돌의 일부를 나타내며 제품의 결과로 발생합니다. 온도의 증가는 주파수 계수와 지수 인자 모두에 영향을 미칩니다.
높은 온도에서 분자는 더 빠르고, 더 강력하게, 더 높은 열 에너지로 이동하여 더 유리한 충돌로 이어집니다.
대부분의 반응에 대 한, 온도 증가 높은 주파수와 기하 급수 요인 결과, 속도 일정 의 상승으로 이어지는, 결과적으로 가속 된 반응 속도 로 번역.

온도 변화가 반응 속도에 미치는 영향

아레니우스 방정식은

많은 화학 반응에 대한 활성화 에너지와 속도 상수 k를 연관시킵니다.

<img alt="Figure1" src="/files/ftp_upload/11698/11698_Equation1.svg" style="text-align: center; height: 30px;">

많은 화학 반응에 대한 활성화 에너지와 속도 상수 k를 연관시킵니다.

 이 방정식에서 R은 값이 8.314 J/mol·K인 이상 기체 상수이고, T는 온도(켈빈), E_a는 활성화 에너지(몰당 줄), e는 상수 2.7183, A는 상수입니다. 충돌 빈도수와 반응 분자의 방향과 관련된 주파수 인자라고 합니다.

주파수 인자 A는 반응 조건이 반응물 분자 사이의 올바른 방향 충돌을 얼마나 잘 선호하는지를 반영합니다. 효과적으로 방향이 지정된 충돌의 확률이 증가하면 A 값이 커지고 반응 속도가 빨라집니다.

지수 항인 e−Eₐ/RT는 활성화 에너지가 반응 속도에 미치는 영향을 설명합니다. 분자 운동 이론에 따르면, 물질의 온도는 구성 원자나 분자의 평균 운동 에너지를 측정한 것입니다. 활성화 에너지가 낮을수록 적절하게 에너지를 받은 분자의 비율이 더 높아지고 반응이 더 빨라집니다.

지수항은 또한 온도가 반응 속도에 미치는 영향을 설명합니다. 더 높은 온도는 활성화 장벽(E_a)을 극복하기에 충분한 에너지(RT)를 보유하는 분자의 더 큰 부분을 나타냅니다. 이는 속도 상수에 대한 더 높은 값을 산출하고 그에 따라 더 빠른 반응 속도를 만들어 냅니다.

반응물이 충돌할 때 생성물을 형성하는 데 필요한 최소 에너지를 활성화 에너지(E_a)라고 합니다. 필요한 활성화 에너지와 반응물 분자 충돌에 의해 제공되는 운동 에너지의 차이는 화학 반응 속도에 영향을 미치는 주요 요인입니다. 활성화 에너지가 분자의 평균 운동 에너지보다 훨씬 크면 빠르게 움직이는 소수의 분자만이 반응할 수 있는 충분한 에너지를 가지므로 반응은 느리게 발생합니다. 활성화 에너지가 분자의 평균 운동 에너지보다 훨씬 작다면, 많은 분자가 적절한 에너지를 갖고 반응이 빠르게 진행될 것입니다.

반응 다이어그램은 관심 있는 반응의 다양한 특성을 설명하기 위해 화학 동역학에서 널리 사용됩니다. 이는 반응이 진행되면서 화학 시스템의 에너지가 어떻게 변화하여 반응물을 생성물로 변환하는지 보여줍니다.

이 문서는 에서 발췌되었습니다<a href="https://openstax.org/books/chemistry-2e/pages/12-5-collision-theory">Openstax, Chemistry 2e, Section 12.5: Collision Theory.</a>

Arrhenius 방정식,

많은 화학 반응에 대한 활성화 에너지와 속도 상수 k를 관련시킵니다.
이 방정식에서 R은 이상 기체 ...

Education

교육

JoVE Core

Organic Chemistry

유기 화학

Unit 1

제1단원

Thermodynamics and Chemical Kinetics

열역학과 화학 반응 속도론

KEY TERMS AND CONCEPTS

주요 용어 및 개념

arrhenius equation in reaction speed

The Arrhenius equation connects activation energy, temperature, and the rate constant, k, for many chemical reactions. It helps explain why some reactions move slowly while others happen faster.

In this equation, R is the ideal gas constant, with a value of 8.314 J/mol·K. T is the temperature in kelvin, Ea is the activation energy in joules per mole, e is the constant 2.7183, and A is the frequency factor.

The frequency factor, A, describes how often reacting molecules collide and how well they are oriented during those collisions. Better orientation increases the chance of effective collisions. That leads to larger A values and faster reaction rates.

The exponential term, e−Ea/RT, shows how activation energy affects the reaction rate. Kinetic molecular theory says that temperature measures the average kinetic energy of atoms or molecules. When activation energy is lower, more molecules have enough energy to react, and the reaction is faster.

The same exponential term also shows the effect of temperature. At higher temperature, a larger fraction of molecules has enough energy, RT, to get over the activation barrier, Ea. This increases the rate constant and speeds up the reaction.

Activation energy is the minimum energy needed to form products during a collision between reactants. If Ea is much larger than the average kinetic energy of the molecules, only a few fast-moving molecules can react, so the reaction is slow. If Ea is much smaller than the average kinetic energy, many molecules can react, so the reaction proceeds quickly.

Reaction diagrams are often used in chemical kinetics to show how a system’s energy changes as reactants turn into products. They help visualize the energy barrier and the path from reactants to products. This text is adapted from Openstax, Chemistry 2e, Section 12.5: Collision Theory.

Arrhenius Equation in Reaction Speed

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The Arrhenius equation connects activation energy, temperature, and the rate constant, k, for many chemical reactions. It helps explain why some reactions move slowly while others happen faster. In this equation, R is the ideal gas constant, with a value of 8.314 J/mol·K. T is the temperature in kelvin, Ea is the activation energy in joules per mole, e is the constant 2.7183, and A is the frequency factor. The frequency factor, A, describes how often reacting molecules collide and how well...

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9-12

3.2.1 9C.3.1.1.2

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Physical Science

SC.912.P.12

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Arrhenius Equation in Reaction Speed

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