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

反応が進行する速度の尺度は、反応速度と呼ばれます。シングルステップ反応の場合、速度は、各反応物または生成物の濃度の経時変化に、対応する化学量論的係数の逆数を掛けたものに等しくなります。時間の経過に伴う濃度の変化は、時間 t での濃度から開始濃度を t で割った値と考えることができます。反応速度は常に正であるため、反応物の発現には負の符号があります。これらの速度は多段階反応では等しくない可能性がありますが、この関係を全体的な反応の推定値として使用できます。
速度の法則、または速度方程式は、反応の速度と反応物濃度との関係を表します。この式では、k は速度定数、A と B は 2 つの反応物、m と n はそれぞれの反応順序です。反応順序は、反応物の濃度と速度との関係を表し、化学量論とは関係ありません。反応順序は、平衡方程式の反応物の係数と同じではないことを覚えておくことが重要です。
反応に2つ以上の反応物が含まれる場合、各反応物の反応順序を考慮する必要があります。全体的な反応順序は、反応物の反応順序の合計に等しくなります。たとえば、反応物 A が 1 次で、反応物 B が 0 次の場合、全体の反応次数は 1 です。単純な反応で最も一般的な反応次数は、ゼロ次、1次、および2次です。一分子反応を例に、それらを見ていきましょう。
反応がゼロ次の場合、反応物濃度は反応速度に影響を与えません。したがって、反応速度は速度定数であるkに等しくなります。濃度に対する反応速度のグラフは水平線です。
一次関係では、反応物濃度は反応速度に線形に関連しています。したがって、速度は、速度定数に反応物濃度を掛けたものに等しくなります。濃度に対する反応速度のグラフは線形になり、kを傾きとします。
反応が2次の場合、濃度と速度の間には二次関係があります。したがって、レートは、レート定数に濃度の2乗を掛けたものに等しくなります。濃度に関する速度のグラフは放物線になり、kを傾きとして使用します。
速度定数kは、反応の活性化エネルギーを反応速度に関連付ける温度依存の値です。これについては、次のラボ実験で探ります。
反応速度は通常、モル/リットル/秒で表されます。反応順序に関係なく、速度の単位は同じです。したがって、速度定数の単位は、反応順序によって異なります。たとえば、Aが1次でBが0次の場合、レート方程式には1リットルあたり1つのモルのインスタンスがあります。したがって、レート定数は逆秒数である必要があります。
では、反応の順序はどのように決定するのでしょうか?反応順序は、一連のテストを使用して実験的に決定する必要があります。反応物が2つある場合、1つの方法は、1つの反応物の濃度を一定に保ち、もう1つの反応物を変化させ、一定量の生成物を作るのにかかる時間を計ることです。同じプロセスが2番目の反応物についても繰り返されます。その後、反応物の濃度の変化に対する速度をプロットし、それがゼロ、1 次、または 2 次のグラフのように見えるかどうかを確認することで、各反応物の順序を推定できます。データを対応するレート方程式と一致させることで、kを計算することもできます。
このラボでは、2 つの反応物の濃度を変化させ、反応が進行して溶液が不透明になるまでの時間を計ることで、2 つの反応物の反応順序を決定します。

濃度依存性

化学反応速度論と反応速度法則
化学反応速度論とは、化学反応の速度または速度を指します。速度は、反応のメカニズム、複雑さ、および反応物の数によって異なります。反応物濃度も反応速度に重要な役割を果たします。
レート法則は、実験を通じてこの関係を定量化します。各反応物は、反応順序と呼ばれる要因によって反応の速度に寄与します。この係数は 0 から 2 の範囲であり、その反応物と反応速度との関係に依存します。
r = k[A]m[B]n for aA + bB + ...→ cC
この式において、rは反応速度、kは反応速度定数、[A]と[B]は反応物AとBの濃度、mとnはそれぞれ反応物AとBの反応順序です。反応速度rは、時間の経過に伴う製品の濃度の変化として定義され、1リットルあたり1秒あたりのモルの単位があります。
<h4>反応の順序</h4>
反応の順序は、反応物の濃度が反応速度に持つ力依存性を表します。全体的な反応順序は、各反応物の反応順序の合計です。反応順序は、平衡化学方程式の化学量論的要因とは関係がないことを覚えておくことが重要です。言い換えれば、化学量論は化学反応の反応順序を決定するために使用することはできません。反応次数は実験的に決定する必要があります
反応順序を決定するために、第2の反応物の濃度は一定に保たれ、第1の反応物の濃度は変化します。反応が起こるのにかかる時間は秒単位で測定されます。ただし、この時間は、反応が完成するまでにかかる時間には対応していません。むしろ、これは反応が始まるのにかかる時間です。次に、さまざまな反応物濃度の反応時間を比較して、順序を決定します。第2の反応物の順序を決定するために、第1の反応物の濃度が一定に保たれ、第2の反応物の濃度が変化するのと同じ一連の反応が行われます。
反応時間を比較することで、反応順序を決定できます。たとえば、反応物濃度が変化しても反応時間が一定のままである場合、反応物は 0 次です。これは、反応速度が反応速度係数kに等しく、M/sの単位を持つ必要があることを意味します。反応時間が濃度の変化に伴って直線的に変化する場合(つまり、濃度を2倍にすると反応時間が2倍になる場合)、反応物は一次です。これは、反応速度が反応速度係数と反応物の濃度の積に等しいことを意味します。この場合、k の単位は 1/s です。最後に、反応物の濃度が2倍になったときに反応時間が4の係数によって影響を受ける場合、反応物は2次です。これは、反応の速度が、速度定数に反応物濃度の2乗を掛けたものに等しくなり、二次関係を形成することを意味します。この場合、kの単位は1/M・sでなければなりません。
反応の全体的な順序は、個々の反応の順序の合計です。たとえば、反応がAに対して一次である場合、m = 1です。そして、反応がBに対してゼロ次である場合、n = 0です。m + n = 1であるため、反応の全体的な順序は1次です。
<h4>反応速度定数</h4>
速度定数kは、反応が実行される反応と温度に固有です。速度定数は、一連の実験から決定されます。測定された速度と初期反応物濃度を使用して、速度方程式を使用して速度定数を解きます。速度定数は温度に依存し、アレニウス方程式によって定義されます。この式は、k と活性化エネルギーE a、温度 T、および理想気体定数 R との関係を表しています。定数Aは比例定数であり、反応物Aと混同しないでください。
<img src="/CDNSource/lm/labs/50/50_Concepts_2.jpg">
<h4>参照</h4>
<ol>
	<li style="font-size:17px">Kotz, J.C., Treichel Jr, P.M., Townsend, J.R. (2012).化学および化学反応性。カリフォルニア州ベルモント:ブルックス/コール、Cengage Learning。</li>
	<li style="font-size:17px">Silderberg, M.S. (2009).化学:物質と変化の分子的性質。マサチューセッツ州ボストン:マグロウヒル。</li>
</ol>

化学反応速度論と反応速度法則
化学反応速度論とは、化学反応の速度または速度を指します。レートはメカニズムによって異なります、...

Education

JoVE Lab Manual

化学

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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chemistry

入門化学ラボコースの指導者と学生のための、包括的でカリキュラムに焦点を当てたビデオ。

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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.

濃度依存性 を教える準備を、この 5 分間の教員向けガイドで行いましょう。JoVE Lab Manual の Chemistry ラボの主要な準備手順を解説します。

Chemistry の 濃度依存性 教員準備 - 2.2K+ 回の視聴 | JoVE Lab Manual

この 10 分間の学生プロトコル動画で、濃度依存性 の手順をステップごとに学びましょう。JoVE Lab Manual の Chemistry コレクションの一部です。

Chemistry の 濃度依存性 学生プロトコル - 4.4K+ 回の視聴 | JoVE Lab Manual

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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