Name: reaction order and rate constants
Uploaded: 2020-03-26T07:22:26.000Z
Duration: 4 min 37 s
Channel: JoVE

K12 Standards

Minnesota Academic Standards in Science

9-12

Chemistry

3.2.1 9C.3.1.1.2

Concentration Dependence

반응이 얼마나 빨리 진행되는지를 측정한 것을 반응 속도라고 합니다. 1단계 반응의 경우, 속도는 시간 경과에 따른 각 반응물 또는 생성물의 농도 변화에 해당 화학량론 계수의 역을 곱한 값과 같습니다. 시간 경과에 따른 농도의 변화는 시간 t에서의 농도에서 시작 농도를 t로 나눈 값으로 생각할 수 있습니다. 반응 속도는 항상 양수이므로 반응물 발현은 음의 부호를 갖습니다. 이러한 비율은 다단계 반응에서 동일하지 않을 수 있지만 이 관계를 전체 반응에 대한 추정치로 사용할 수 있습니다.
속도 법칙 또는 속도 방정식은 반응 속도와 반응물 농도 사이의 관계를 설명합니다. 이 방정식에서 k는 속도 상수, A와 B는 두 반응물, m과 n은 각각의 반응 순서입니다. 반응 순서는 반응물의 농도와 속도 사이의 관계를 설명하며 화학량론과 관련이 없습니다. 반응 순서는 균형 방정식에서 반응물의 계수와 동일하지 않다는 것을 기억하는 것이 중요합니다.
반응에 두 개 이상의 반응물이 포함된 경우 각 반응물에 대한 반응 순서를 고려해야 합니다. 전체 반응 순서는 반응물의 반응 순서의 합과 같습니다. 예를 들어, 반응물 A가 1차이고 반응물 B가 0차인 경우 전체 반응 차수는 1입니다. 단순 반응에서 가장 일반적인 반응 순서는 0차, 1차 및 2차입니다. 단분자 반응을 예로 들어 살펴보겠습니다.
반응이 0차수인 경우 반응물 농도는 반응 속도에 영향을 미치지 않습니다. 따라서 반응 속도는 속도 상수인 k와 같습니다. 농도에 대한 반응 속도의 그래프는 수평선입니다.
1차 관계에서 반응물 농도는 반응 속도와 선형적으로 관련됩니다. 따라서, 속도는 속도 상수 곱하기 반응물 농도와 같습니다. 농도에 대한 반응 속도의 그래프는 선형이며 k를 기울기로 합니다.
반응이 2차인 경우 농도와 속도 사이에 2차 관계가 있습니다. 따라서 속도는 속도 상수에 농도의 제곱을 곱한 값과 같습니다. 농도에 대한 비율의 그래프는 포물선이며 k는 기울기입니다.
속도 상수 k는 반응의 활성화 에너지를 반응 속도와 관련시키는 온도 종속 값입니다. 다음 실습 실험에서 이를 살펴보겠습니다.
반응 속도는 일반적으로 초당 리터당 몰로 표시됩니다. 속도는 반응 순서에 관계없이 동일한 단위를 갖습니다. 따라서 속도 상수는 반응 순서에 따라 다른 단위를 갖습니다. 예를 들어, A가 1차이고 B가 0차인 경우 속도 방정식에 리터당 몰의 인스턴스가 하나 있습니다. 따라서 속도 상수는 역초 단위여야 합니다.
그렇다면 반응 순서는 어떻게 결정할까요? 반응 순서는 일련의 테스트를 사용하여 실험적으로 결정해야 합니다. 두 개의 반응물이 있는 경우 한 반응물의 농도를 일정하게 유지하고 다른 반응을 변화시키며 일정량의 생성물을 만드는 데 걸리는 시간을 측정하는 것입니다. 두 번째 반응물에 대해서도 동일한 과정이 반복됩니다. 그런 다음 반응물의 다양한 농도에 대한 속도를 표시하고 0, 1차 또는 2차 그래프처럼 보이는지 확인하여 각 반응물의 순서를 추정할 수 있습니다. 데이터를 해당 비율 방정식과 일치시키면 k도 계산할 수 있습니다.
이 실험실에서는 농도를 변화시키고 반응이 용액을 불투명하게 만드는 데 걸리는 시간을 측정하여 두 반응물의 반응 순서를 결정합니다.

집중 의존성

화학 역학과 반응 속도 법칙
화학 반응 속도학은 화학 반응의 속도 또는 속도를 나타냅니다. 속도는 반응의 메커니즘, 복잡성 및 반응물의 수에 따라 다릅니다. 반응물 농도는 또한 반응 속도에 중요한 역할을 합니다.
비율 법칙은 실험을 통해 이 관계를 정량화합니다. 각 반응물은 반응 순서(reaction order)로 알려진 요인에 의해 반응 속도에 기여합니다. 이 계수의 범위는 0에서 2까지 다양할 수 있으며 해당 반응물과 반응 속도의 관계에 따라 다릅니다.
r = k[A]m[B]n for aA + bB + ... → cC
이 식에서, r은 반응 속도, k는 반응 속도 상수, [A] 및 [B]는 반응물 A와 B의 농도, m과 n은 각각 반응물 A와 B의 반응 순서입니다. 반응 속도 r은 시간에 따른 생성물 농도의 변화로 정의되며 초당 리터당 몰 단위를 갖습니다.
<h4>반응의 순서</h4>
반응의 순서는 반응물의 농도가 반응 속도에 미치는 전력 의존성을 설명합니다. 전체 반응 순서는 각 반응물에 대한 반응 순서의 합입니다. 반응 순서는 균형 잡힌 화학 방정식의 화학량론적 요인과 관련이 없다는 것을 기억하는 것이 중요합니다. 즉, 화학량론은 화학 반응에 대한 반응 순서를 결정하는 데 사용할 수 없습니다. 반응 순서는 실험적으로 결정해야 합니다.
반응 순서를 결정하기 위해 두 번째 반응물의 농도는 일정하게 유지되는 반면 첫 번째 반응물의 농도는 변합니다. 반응이 발생하는 데 걸리는 시간은 초 단위로 측정됩니다. 그러나 이 시간은 반응이 완료되는 데 걸리는 시간과 일치하지 않습니다. 대신, 이것은 반응이 시작되는 데 걸리는 시간입니다. 그런 다음 서로 다른 반응물 농도에 대한 반응 시간을 비교하여 순서를 결정합니다. 두 번째 반응물의 순서를 결정하기 위해 동일한 일련의 반응이 수행되며, 여기서 첫 번째 반응물의 농도는 일정하게 유지되고 두 번째 반응물의 농도는 변합니다.
반응 시간을 비교하여 반응 순서를 결정할 수 있습니다. 예를 들어, 반응물 농도의 변화에도 불구하고 반응 시간이 일정하게 유지되면 반응물은 0차입니다. 이는 반응 속도가 반응 속도 계수 k와 동일하며 단위가 M/s여야 함을 의미합니다. 반응 시간이 농도 변화에 따라 선형적으로 변하는 경우(즉, 농도를 두 배로 늘리면 반응 시간에 2배의 영향을 미침) 반응물은 1차입니다. 이는 반응 속도가 반응 속도 계수와 반응물의 농도의 곱과 같다는 것을 의미합니다. 이 경우 k의 단위는 1/s입니다. 마지막으로, 반응물의 농도가 두 배가 될 때 반응 시간이 4의 요인에 의해 영향을 받는 경우, 반응물은 2차입니다. 이것은 반응 속도가 속도 상수에 반응물 농도의 제곱을 곱한 것과 같아 2차 관계를 형성한다는 것을 의미합니다. 이 경우 k의 단위는 1/M⋅s여야 합니다.
반응의 전체 순서는 개별 반응 순서의 합입니다. 예를 들어, 반응이 A에 대해 1차인 경우 m = 1입니다. 그리고 반응이 B에 대해 0차수이면 n = 0입니다. m + n = 1이므로 반응의 전체 순서는 1차입니다.
<h4>반응 속도 상수</h4>
속도 상수 k는 반응 및 반응이 수행되는 온도에 따라 다릅니다. 속도 상수는 일련의 실험에서 결정됩니다. 측정된 속도와 초기 반응물 농도를 사용하여 속도 방정식을 사용하여 속도 상수를 해석합니다. 속도 상수는 온도에 따라 달라지며 Arrhenius 방정식에 의해 정의됩니다. 이 방정식은 k와 활성화 에너지 E,a, 온도 T, 이상 기체 상수 R 사이의 관계를 설명합니다. 상수 A는 비례 상수이며 반응물 A와 혼동해서는 안 됩니다.
<img src="/CDNSource/lm/labs/50/50_Concepts_2.jpg">
<h4>참조</h4>
<ol>
	<li style="font-size:17px">Kotz, J.C., Treichel Jr, P.M., Townsend, J.R. (2012). 화학 및 화학 반응성. 캘리포니아 벨몬트 : Brooks / Cole, Cengage Learning.</li>
	<li style="font-size:17px">Silderberg, M.S. (2009). 화학: 물질과 변화의 분자적 성질. 매사추세츠주 보스턴: 맥그로 힐.</li>
</ol>

화학 역학과 반응 속도 법칙
화학 반응 속도학은 화학 반응의 속도 또는 속도를 나타냅니다. 비율은 메커니즘에 따라 다릅니다.

Education

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JoVE Lab Manual

화학

reaction order and rate constants

Chemical kinetics describes the speed of a chemical reaction. The rate depends on the reaction mechanism, the complexity of the reaction, and the number of reactants involved. Reactant concentration also affects how fast a reaction happens. The rate law is the experimental relationship that connects these factors to reaction rate.

In the rate law, each reactant contributes through a reaction order. The general form is r = k[A]^m[B]^n for aA + bB + ... → cC. Here, r is the reaction rate, k is the rate constant, and [A] and [B] are the reactant concentrations. The exponents m and n show the reaction order for each reactant.

The reaction rate is the change in product concentration over time. Its units are moles per liter per second. The overall reaction order is the sum of the individual orders. Reaction order is not the same as the numbers in the balanced chemical equation, so stoichiometric coefficients cannot be used to find it. Reaction orders must be measured experimentally.

To find a reaction order, one reactant concentration is changed while the other is held constant. The reaction time is measured in seconds, but this is the time for the reaction to start, not the time to completion. The times from different concentrations are compared to determine the order. The same process is repeated for the second reactant by switching which concentration is varied.

If the reaction time stays the same even when concentration changes, the reactant is zero-order. In that case, the rate equals k, and k has units of M/s. If the time changes linearly with concentration, the reactant is first order. Then the rate equals k times the reactant concentration, and k has units of 1/s. If doubling the concentration changes the time by a factor of 4, the reactant is second order. Then the rate equals k times the square of the concentration, and k has units of 1/M·s.

The overall order is the sum of the individual orders. For example, if A is first order and B is zero-order, the total order is first order because m + n = 1. The rate constant, k, is specific to the reaction and the temperature used. It is found from the experimental data by using the measured rate and initial concentrations in the rate equation.

The rate constant also depends on temperature through the Arrhenius equation. This equation relates k to activation energy, Ea, temperature, T, and the ideal gas constant, R. The constant A in the equation is a proportionality constant. It should not be confused with reactant A.

Reaction Order and Rate Constants

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concentration dependence

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Reaction Rate, Arrhenius, and Catalysts

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Boiling Point and Vapor Pressure

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Purifying Crystals by Solubility

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extraction

Separating Mixtures with Solvent Extraction

Solvent extraction is a common way to separate and isolate a target compound in organic chemistry. In this process, a solute moves from one phase to another so it can be separated from unreacted starting materials or impurities. Extraction is also useful when a product is dissolved in a reaction solvent that is hard to remove by evaporation, such as a solvent with a high boiling point. There are three main types of extraction. In solid-liquid extraction, the solute moves from a solid phase...

simple distillation

Separating Liquids by Boiling Point

Separating liquids by boiling point is the goal of distillation. A miscible mixture contains liquids that mix evenly, and it can be heated so that the more volatile liquid evaporates first. Volatility is a liquid’s tendency to vaporize, and boiling begins when bubbles form in the liquid phase. In a closed container, liquid and vapor can reach equilibrium, which means the rate of vaporization equals the rate of condensation. The pressure from the vapor above the liquid is called vapor pressure.

steam distillation

Steam Distillation and Low-Boiling Separation

Steam distillation is a separation method for temperature-sensitive organic compounds. It works best when the organic compound is immiscible in water, meaning the two liquids do not mix. The method helps remove the organic molecule from a non-volatile contaminant without using the higher temperatures needed for many other separations. In steam distillation, the immiscible mixture is heated until both water and the volatile organic compound distill together. The vapor rises to a condenser,...

thin-layer chromatography

TLC Separation by Polarity

Thin-layer chromatography (TLC) separates compounds in a mixture by polarity. It uses the same basic parts as other chromatography methods: a stationary phase, a mobile phase, and the solute. In TLC, the stationary phase is a thin coating on a plate instead of material packed into a column. The stationary phase in most TLC systems is polar silica gel, a form of silicon dioxide. Its surface has OH groups that can form hydrogen bonds. The sample is first spotted on a pencil start line with a...

column chromatography

Separating Mixtures by Polarity

Column chromatography separates compounds in an organic chemistry lab by using differences in physical properties. It is especially useful for microscale separations when less than 10 grams of material is available for analysis. The method can separate a mixture based on solubility, polarity, hydrophobicity, size, and charge. Any chromatography system has three main parts: the stationary phase, the mobile phase, and the sample mixture. In column chromatography, the stationary phase is usually...

hydrolysis of an ester

Soap Formation from Triglycerides

Triglycerides are lipids made of a glycerol backbone linked to three fatty acids. They are common in vegetable oils and animal fats. Plant lipids are the basis of vegetable oils, while animal lipids are used as lard or general sources of fats. A fatty acid has a long carbon chain, usually between 12 and 20 carbons, with a weak organic acid at one end. Some fatty acids contain double bonds. These are unsaturated fats. The double bond usually gives the chain a bent, cis shape. As a result,...

synthesis of luminol

Luminol Chemiluminescence in Forensics

Luminol chemiluminescence shows how a chemical reaction can produce light and help with blood detection. Chemical reactions may be endothermic or exothermic, depending on whether they absorb or release heat as reactants become products. The enthalpy of a reaction is the energy difference between reactants and products, or ΔH. A positive ΔH means the reaction is endothermic. A negative ΔH means it is exothermic. Many reactions do not happen in a single step. They can pass through intermediates...

esterification

Ester Formation and Everyday Fragrances

Esters are organic compounds with a carbonyl group attached to an oxygen that connects to another alkyl or aryl group. Their general formula is RCOOR'. They are often made by reacting a carboxylic acid with an alcohol in an esterification reaction. In this process, the hydroxyl group of the acid is replaced by an alkyl or aryl group. Many simple esters have familiar fruit and flower smells because their structures are small and less complex. Formic acid and methanol can combine to form methyl...

identification of unknown aldehydes and ketones

identification-of-unknown-aldehydes-and-ketones

Carbonyl Tests for Aldehydes and Ketones

Aldehydes and ketones are carbonyl compounds, which means they contain a C=O functional group. A ketone has two alkyl or aryl groups attached to the carbonyl carbon. Acetone is the simplest ketone, with two methyl groups. An aldehyde is similar, but it has at least one hydrogen attached to the carbonyl carbon. Formaldehyde is the simplest aldehyde, and acetaldehyde has one hydrogen and one methyl group. The carbonyl carbon in both aldehydes and ketones is electrophilic because the oxygen atom...

uv-vis spectroscopy of dyes

How Dyes Absorb Visible Light

Dyes absorb visible light because their molecular structure lets them interact with specific wavelengths. When light hits a substance, some light is absorbed and the rest is reflected or transmitted. The color we see depends on the wavelength that is reflected. A blue substance reflects blue light, around 430 to 480 nm, and absorbs the complementary orange region, around 590 to 630 nm. Compounds that do not absorb in the visible range appear colorless to the human eye. Light also has energy and...

identifying alcohols

Alcohol Tests for Primary, Secondary, and Tertiary

Alcohol tests can help sort alcohols by structure and reactivity. Alcohols are organic molecules with a hydroxyl group attached to an alkyl or aryl group, written as ROH. If the carbon with the hydroxyl group has one R group, the alcohol is primary. If it has two R groups, it is secondary. If it has three R groups, it is tertiary. Alcohols can also be aromatic when they contain a benzene ring. Phenol is the simplest aromatic alcohol. To identify an alcohol, chemists can use its chemical...

chemistry

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Learn how concentration affects reaction rate, how to determine zero-, first-, and second-order reactions, and how rate constants depend on temperature.

Reaction Order and Rate Constants | JoVE K12

Alabama Course of Study Science

Matter and Its Interactions: Energy

9-12.C.3.3.d

Next Generation Science Standards

High School

Physical Science

Matter and Its Interactions

HS-PS1-5

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-5.

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Molecular Orbital (MO) Theory

Source: Tamara M. Powers, Department of Chemistry, Texas A&#38;M University
This protocol serves as a guide in the synthesis of two metal complexes ...

Electron Behavior

Electrons are negatively charged subatomic particles that are attracted to an orbit around the positively-charged nucleus of an atom. They reside in ...

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

Effect of Temperature Change on Reaction Rate

The Arrhenius equation,

relates the activation energy and the rate constant, k, for many chemical reactions.
In this equation, R is the ideal gas ...

factors-influencing-the-rate-of-chemical-reactions

Factors Influencing the Rate of Chemical Reactions

A variety of factors influence the rate of chemical reactions. For a chemical reaction to happen, atoms must collide with enough energy to overcome the ...

Concentration and Rate Law

The rate of a reaction is affected by the concentrations of reactants. Rate laws (differential rate laws) or rate equations are mathematical expressions ...

Measuring Reaction Rates

Polarimetry finds application in chemical kinetics to measure the concentration and reaction kinetics of optically active substances during a chemical ...

Temperature Dependence

Chemical Kinetics 
The reaction rate is the speed at which a chemical reaction occurs. The reaction rate is defined as the change in concentration of a ...

Reaction Rate

The rate of reaction is the change in the amount of a reactant or product per unit time. Reaction rates are therefore determined by measuring the time ...

Chemical Kinetics and the Reaction Rate Law
Chemical kinetics refers to the rate or speed of a chemical reaction. The rate depends on the mechanism, ...

Matter and Its Interactions: Develop a model based on evidence to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy. (P: 2, CC: 5, CI: PS1)

Solution Formation

There is no one solvent that can dissolve every type of solute. Some substances that readily dissolve in a certain solvent might be insoluble in a ...

Energetics of Solution Formation

The formation of a solution is an example of a spontaneous process, which is a process that occurs under specified conditions without energy from some ...

General Properties of Solutions

Many common substances around us exist as a solution, such as ocean water, air, and gasoline. All solutions are mixtures of substances that are composed ...

Solutions and Concentrations

Source: Laboratory of Dr. Michael Evans &#8212; Georgia Institute of Technology
A solution is a homogeneous mixture containing some components in small ...

Solubility

Solubility
Solubility describes how much of a solute can dissolve in a given volume of a specific solvent. Solubility is usually reported in terms of ...

Solution, Solubility, and Solubility Equilibrium
A solution is a homogeneous mixture&#160;composed of a solvent, the major component, and a solute, the ...

Solution Equilibrium and Saturation

Imagine adding a small amount of sugar to a glass of water, stirring until all the sugar has dissolved, and then adding a bit more. You can repeat this ...

Intermolecular Forces in Solutions

The formation of a solution is an example of a spontaneous process, a process that occurs under specified conditions without energy from some external ...

Matter and Its Interactions: Develop models to illustrate the changes in the composition of the nucleus of the atom and the energy released during the processes of fission, fusion, and radioactive decay. (P: 2, CC: 5, CI: PS1)

9C.3.1.1.3

Chemical and Solubility Equilibria

The free energy change associated with dissolving a solute in a liter of solvent is called the free energy of a solution, &#916;Gsolution. The overall ...

Matter and Its Interactions: Apply scientific principles and evidence to provide an explanation about the effects of changing the surface area, agitation, temperature, and concentration of the reacting particles on the rate at which the reaction occurs. (P: 6, CC: 1, CI: PS1)

9C.3.2.1.2

3 Developing possible explanations of phenomena or designing solutions to engineering problems
 3.2 Constructing explanations and designing solutions 
  3.2.1 Students will be able to apply scientific principles and empirical evidence (primary or secondary) to explain the causes of phenomena or identify weaknesses in explanations developed by the students or others.

Reaction Order and Rate Constants

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