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

Мера того, насколько быстро протекает реакция, называется скоростью реакции. Для одноступенчатой реакции скорость равна изменению концентрации каждого реагента или продукта с течением времени, умноженному на обратный соответствующий стехиометрический коэффициент. Изменение концентрации с течением времени можно представить себе как концентрацию в момент времени t за вычетом начальной концентрации, деленной на t. Скорость реакции всегда положительная, поэтому реагентные выражения имеют отрицательные знаки. Эти скорости могут быть неравны в многоступенчатых реакциях, но мы все равно можем использовать эту зависимость в качестве оценки для общей реакции.
Закон скорости, или уравнение скорости, описывает соотношение между скоростью реакции и концентрацией реагентов. В этом уравнении k — константа скорости, A и B — два реагента, а m и n — соответствующие порядки реакций. Порядок реакции описывает взаимосвязь между концентрацией реагента и скоростью и не связан со стехиометрией. Важно помнить, что порядок реакции не совпадает с коэффициентом реагента в сбалансированном уравнении.
Когда в реакции участвуют два или более реагента, мы должны учитывать порядок реакции для каждого из них. Общий порядок реакции равен сумме порядков реакции реагентов. Например, если реагент А является веществом первого порядка, а реагент В — нулевым порядком, то общий порядок реакции равен единице. Наиболее распространенными порядками реакций в простых реакциях являются нулевые, первого и второго порядка. Давайте рассмотрим их на примере одномолекулярной реакции.
Если реакция нулевого порядка, то концентрация реагента не влияет на скорость реакции. Таким образом, скорость реакции равна k, постоянной скорости. График скорости реакции по отношению к концентрации представляет собой горизонтальную линию.
В соотношении первого порядка концентрация реагента линейно связана со скоростью реакции. Таким образом, скорость равна константе скорости, умноженной на концентрацию реагента. График скорости реакции по отношению к концентрации будет линейным, с k в качестве наклона.
Если реакция второго порядка, то существует квадратичная зависимость между концентрацией и скоростью. Таким образом, скорость равна константе скорости, умноженной на квадрат концентрации. График скорости по отношению к концентрации будет параболическим, где k будет наклоном.
Константа скорости, k, является зависящей от температуры величиной, которая связывает энергию активации реакции со скоростью реакции. Вы узнаете об этом в следующем лабораторном эксперименте.
Скорость реакции обычно указывается в молях на литр в секунду. Скорость имеет одинаковые единицы, независимо от порядка реакции. Таким образом, константа скорости имеет разные единицы измерения, в зависимости от порядка реакции. Например, если A — это первый порядок, а B — нулевой порядок, то в уравнении скорости мы имеем один экземпляр молей на литр. Следовательно, константа скорости должна быть обратной в секундах.
Так как же мы определяем порядок реакции? Порядок реакции должен быть определен экспериментально с помощью серии тестов. Если у вас есть два реагента, один из методов заключается в том, чтобы поддерживать концентрацию одного реагента постоянной, изменять другой и измерять время, необходимое для производства определенного количества продукта. Тот же процесс повторяется для второго реагента. Затем вы можете оценить порядок для каждого реагента, построив график скорости в зависимости от изменяющейся концентрации реагентов и увидев, выглядит ли он как график нулевого, первого или второго порядка. Сопоставление ваших данных с соответствующим уравнением скорости также позволит вам вычислить k.
В этой лабораторной работе вы определите порядок реакции двух реагентов, изменяя их концентрацию и замеря, сколько времени требуется для того, чтобы реакция протекала до превращения раствора в непрозрачный.

Зависимость от концентрации

Химическая кинетика и закон скорости реакции
Химическая кинетика относится к скорости или скорости химической реакции. Скорость зависит от механизма, сложности и количества реагентов в реакции. Концентрация реагента также играет значительную роль в скорости реакции.
Закон скорости количественно определяет эту зависимость с помощью экспериментов. Каждый реагент вносит свой вклад в скорость реакции с помощью фактора, известного как порядок реакции. Этот фактор может варьироваться от нуля до двух, и это зависит от отношения этого реагента к скорости реакции.
r = k[A]m[B]n for aA + bB + ... → сК
В этом уравнении r — скорость реакции, k — константа скорости реакции, [A] и [B] — концентрации реагентов A и B, а m и n — порядки реакции реакций A и B соответственно. Скорость реакции, r, определяется как изменение концентрации продукта со временем и имеет единицы измерения молей на литр в секунду.
<h4>Порядок реакции</h4>
Порядок реакции описывает зависимость мощности концентрации реагентов от скорости реакции. Общий порядок реакции представляет собой сумму порядков реакции для каждого из реагентов. Важно помнить, что порядок реакции НЕ связан со стехиометрическими факторами сбалансированного химического уравнения. Другими словами, стехиометрия не может быть использована для определения порядка реакции в химической реакции. Порядок реакции должен быть определен экспериментальным путем
Для определения порядка реакции концентрацию второго реагента держат постоянной, в то время как концентрация первого реагента варьируется. Время, необходимое для возникновения реакции, измеряется секундами; Однако это время не соответствует времени, которое требуется для того, чтобы реакция дошла до завершения. Вместо этого это время, необходимое для начала реакции. Время реакции для различных концентраций реагентов затем сравнивается для определения порядка. Тот же ряд реакций выполняется для определения порядка второго реагента, где концентрация первого реагента остается постоянной, а концентрация второго реагента варьируется.
Сравнивая время реакции, можно определить порядок реакции. Например, если время реакции остается постоянным, несмотря на изменения концентрации реагента, то реагент имеет нулевой порядок. Это означает, что скорость реакции равна коэффициенту скорости реакции, k, который должен иметь единицы M/s. Если время реакции изменяется линейно с изменением концентрации (т.е. удвоение концентрации влияет на время реакции в 2 раза), то реагент первого порядка. Это означает, что скорость реакции равна произведению коэффициента скорости реакции на концентрацию реагента. В этом случае k имеет единицы измерения 1/с. Наконец, если время реакции изменяется в 4 раза, когда концентрация реагента удваивается, то реагент имеет второй порядок. Это означает, что скорость реакции равна константе скорости, умноженной на квадрат концентрации реагента, образуя квадратичное соотношение. В этом случае единицы k должны быть равны 1/M⋅s.
Общий порядок реакции представляет собой сумму отдельных порядков реакции. Например, если реакция первого порядка по отношению к А, то m = 1. А если реакция нулевого порядка по отношению к В, то n = 0. Общий порядок реакции — первый порядок, потому что m + n = 1.
<h4>Скорость реакции постоянна</h4>
Константа скорости, k, специфична для реакции и температуры, при которой она протекает. Константа скорости определяется по результатам серии экспериментов. Используя измеренную скорость и начальные концентрации реагентов, уравнение скорости используется для расчета постоянной скорости. Константа скорости зависит от температуры и определяется уравнением Аррениуса. Это уравнение описывает соотношение между k и энергией активации Ea, температурой T и постоянной идеального газа R. Константа А является константой пропорциональности, и ее не следует путать с реагентом А.
<img src="/CDNSource/lm/labs/50/50_Concepts_2.jpg">
<h4>Ссылки</h4>
<ol>
	<li style="font-size:17px">Kotz, J.C., Treichel Jr, P.M., Townsend, J.R. (2012). Химия и химическая реакционная способность. Бельмонт, Калифорния: Брукс/Коул, Cengage Learning.</li>
	<li style="font-size:17px">Silderberg, M.S. (2009). Химия: молекулярная природа материи и изменения. Бостон, Массачусетс: Макгроу Хилл.</li>
</ol>

Химическая кинетика и закон скорости реакции
Химическая кинетика относится к скорости или скорости химической реакции. Курс зависит от механизма,...

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JoVE Lab Manual

Химия

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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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

Comprehensive, curriculum-focused videos for both instructors and students in introductory chemistry lab courses.

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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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