Name: catalyst action in reaction rates
Uploaded: 2020-09-24T15:06:50.000Z
Duration: 2 min 50 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.5.1

Catalysis

연구자들은 반응 메커니즘과 동력학에 대한 연구를 진행하여 반응 속도를 최적화합니다. 온도나 농도가 증가하면 속도가 빨라지지만 너무 많이 증가하면 분해나 부산물 생성으로 이어질 수도 있습니다. 다른 대안으로는 영구적으로 변경되거나 소실되지 않고 반응 속도를 가속화하는 화학 물질을 반응 혼합물에 추가할 수 있습니다.

이러한 물질들은 촉매라고 불리며 활성화 에너지를 변경하는 방식으로 속도 상수에 영향을 미칩니다. 활성화 에너지가 높을수록 반응 속도가 느려진다는 점을 기억하십시오. 따라서, 액상 과산화수소의 분해와 같은 많은 화학 반응들은 느리게 진행됩니다.

촉매를 추가하면 반응물과 생성물의 에너지 상태에 영향을 주지 않는 대체 반응 메커니즘을 제공하여 활성화 에너지를 낮춥니다. 촉매에는 두 가지 유형, 균일 촉매와 불균일 촉매가 있습니다. 균일 촉매는 반응물과 동일한 단계에 존재합니다.

예를 들어, 브롬화나트륨을 액상 과산화수소에 첨가하여 기체 산소와 물로의 분해를 가속화합니다. 먼저, 브롬화 이온은 산성 매질 속의 과산화수소와 반응하여 오랜지 색의 수용성 브롬 용액과 물을 형성합니다. 다음으로, 수용성 브롬과 과산화수소가 반응하여 무색의 용액인 브롬화 이온을 방출합니다.

촉매의 특성상 브롬화 이온은 반응을 가속화하지만 소실되지 않으며 순 균형 방정식에 나타나지 않습니다. 불균일 촉매는 반응물에 비해 다른 물리적 상태로 존재합니다. 불균일 촉매는 흡착, 확산, 반응 및 탈착의 네 가지 기본 단계로 특징지어집니다.

예를 들어, 에탄에 대한 불포화 에틸렌 기체의 수소화 반응은 숯에 미세하게 분산된 팔라듐에 의해 가속화됩니다. 여기, 촉매는 고체 상태로 존재하지만 반응물은 기체 형태로 존재합니다. 이런 불균일 촉매의 작용에 의해 에틸렌과 수소 분자는 촉매 표면에 흡착합니다.

수소-수소 결합이 깨져 수소 원자가 촉매 표면에서 확산되도록 합니다. 확산되는 수소 원자가 흡착된 에탄 분자와 부딪치면 반응하여 포화 에탄을 형성합니다. 그 다음 생성물이 금속 표면에서 탈착하여 금속 표면에서 멀어지게 되고 촉매 자체만 남게 됩니다.

촉매작용

촉매의 존재는 화학 반응 속도에 영향을 미칩니다. 촉매는 공정 중에 소모되지 않고 반응 속도를 높일 수 있는 물질입니다. 화학반응에서 촉매의 역할에 대한 기본적인 이해는 반응 메커니즘의 개념과 에너지 다이어그램을 통해 이해할 수 있습니다.

<img alt="Image1" src="/files/ftp_upload/11383/11383_Image_1.png" style="text-align: center; height: 350px;" />

예시된 이미지는 촉매가 없는 경우(빨간색 곡선)와 존재하는 경우(파란색 곡선) 진행되는 흡열 화학 공정에 대한 반응 다이어그램을 나타냅니다.

두 곡선 모두 동일한 전체 반응을 나타냅니다. 즉, 동일한 에너지에서 시작하고 끝납니다. (이 경우 생성물은 반응물보다 더 많은 에너지를 갖습니다. 따라서 반응은 흡열입니다.) 그러나 반응 메커니즘은 다릅니다. 촉매되지 않은 반응은 1단계 메커니즘을 통해 진행됩니다(단 하나의 전이 상태만 관찰됨). 대조적으로, 촉매 반응은 활성화 에너지가 현저히 낮은 2단계 메커니즘(두 개의 전이 상태가 관찰됨)을 따릅니다. 반응 경로의 이러한 차이는 활성화 에너지가 낮은 대체 반응 메커니즘을 제공하여 반응을 가속화하는 촉매의 역할을 보여줍니다.

촉매 반응 메커니즘은 비촉매 메커니즘보다 더 많은 수의 기본 단계를 포함할 필요가 없습니다. 그러나 속도 결정 단계가 더 빠른(낮은 E_a 또는 활성화 에너지를 사용하여) 대체 반응 경로를 제공해야 합니다.

촉매 반응은 촉매 공정 동안 촉매와 반응물이 존재하는 물리적 상태에 따라 균질 또는 불균일로 분류될 수 있습니다.

균질한 촉매작용

균일 촉매작용에서 촉매는 반응물(고체, 액체 또는 기체)과 동일한 상에 존재합니다. 공정 중에 촉매는 반응물과 상호작용하여 중간 물질을 형성하고, 이 중간 물질은 하나 이상의 단계에서 분해되거나 다른 반응물과 반응하여 원래의 촉매를 재생하고 최종 생성물을 형성합니다.

균질 촉매작용의 예로는 지구의 상부 대기에서 발생하는 오존 분해와 관련된 화학적 과정이 있습니다. 오존은 분해되어 이원자 산소를 생성하는 비교적 불안정한 분자입니다. 이 분해 반응은 다음과 같은 2단계 메커니즘과 일치합니다.

<img alt="Eq1" src="/files/ftp_upload/11383/11383_Equation_1.png" style="text-align: center; height: 75px;" />

많은 물질이 오존 분해를 촉매할 수 있습니다. 예를 들어, 산화질소에 의한 오존 분해는 다음과 같은 3단계 메커니즘을 통해 발생하는 것으로 여겨집니다.

<img alt="Eq2" src="/files/ftp_upload/11383/11383_Equation_2.png" style="text-align: center; height: 115px;" />

그러나 전체 반응은 2단계 비촉매 메커니즘과 3단계 NO 촉매 메커니즘 모두에서 동일합니다.

<img alt="Eq3" src="/files/ftp_upload/11383/11383_Equation_3.png" style="text-align: center; height: 50px;" />

촉매 반응에서 NO는 메커니즘의 첫 번째 단계에서는 반응물이고 마지막 단계에서는 생성물이라는 점에 유의하세요. 이는 촉매의 또 다른 특징입니다. 화학 반응에 참여하지만 반응에 의해 소모되지는 않습니다. 또한, 이 균질 촉매작용에서는 반응물과 촉매가 모두 기체상으로 존재합니다.

<img alt="Image2" src="/files/ftp_upload/11383/11383_Image_2.png" style="text-align: center; height: 250px;" />

불균일 촉매작용에서 촉매는 반응물과 다른 상(보통 고체)으로 존재합니다. 이러한 촉매는 일반적으로 반응이 일어날 수 있는 활성 표면을 제공함으로써 기능합니다. 불균일 촉매에 의해 촉매되는 기체 및 액체상 반응은 기체 또는 액체상 내부가 아닌 촉매 표면에서 발생합니다.

이종 촉매작용은 일반적으로 다음 과정을 포함합니다.

<ol>
	<li>촉매 표면의 반응물 흡착</li>
	<li>흡착된 반응물의 활성화</li>
	<li>흡착된 반응물의 반응</li>
	<li>촉매 표면에서 생성물의 탈착</li>
</ol>

그림 이미지는 고체 니켈 표면에서 에텐과 수소 가스의 불균일 촉매작용을 포함하는 반응 메커니즘을 나타내며, 에탄 가스(C_2H_4 + H_2 ⟶ C_2H_6)를 형성합니다.

(a) 수소는 니켈 표면에 흡착됩니다. 이 과정에서 수소-수소 결합이 끊어져 니켈-수소 결합이 형성됩니다.

(b) 에텐은 또한 탄소-탄소 파이 결합을 끊고 니켈-탄소 결합을 형성함으로써 니켈 표면에 흡착합니다.

(c) 수소 원자는 표면 전체로 확산되어 충돌하여 에탄(C_2H_6)을 형성할 때 새로운 탄소-수소 결합을 형성합니다.

(d) 에탄 분자는 니켈 표면에서 탈착됩니다.

이종 촉매작용은 암모니아, 질산, 황산, 메탄올과 같은 화학 제품을 산업적으로 제조하는 데 사용됩니다. 이종 촉매는 대부분의 가솔린 구동 자동차에 사용되는 촉매 변환기에도 사용됩니다.

이 문서는 에서 발췌되었습니다 <a href="https://openstax.org/books/chemistry-2e/pages/12-7-catalysis">Openstax, Chemistry 2e, Section 12.7: Catalysis</a>.

촉매의 존재는 화학 반응 속도에 영향을 미칩니다. 촉매는 소비되지 않고 반응 속도를 높일 수 있는 물질입니다 ...

Education

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JoVE Core

화학

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Chemical Kinetics

화학 반응 속도론

KEY TERMS AND CONCEPTS

주요 용어 및 개념

catalyst action in reaction rates

Catalysts change the rate of a chemical reaction by giving it a faster path. A catalyst increases reaction rate without being consumed during the process. Its effect is often explained with reaction mechanisms and energy diagrams.

For an endothermic reaction, the reactants and products start and end at the same energies in both cases. The uncatalyzed path is a one-step mechanism with one transition state. The catalyzed path follows a different mechanism with two transition states and a lower activation energy, or Ea. The lower rate-determining barrier is what makes the reaction faster.

Catalytic reactions are often grouped as homogeneous or heterogeneous. In homogeneous catalysis, the catalyst and reactants are in the same phase, which may be solid, liquid, or gas. The catalyst reacts with the reactant to form an intermediate, and that intermediate then breaks down or reacts again to form the product and regenerate the catalyst.

A good example of homogeneous catalysis is ozone decomposition in the upper atmosphere. Ozone breaks down to form diatomic oxygen, and nitric oxide can catalyze that process through a three-step mechanism. In this reaction, NO appears as a reactant in the first step and a product in the last step, which shows that it participates in the reaction but is not used up. Here, both the reactant and the catalyst are gases.

In heterogeneous catalysis, the catalyst is in a different phase from the reactants, usually a solid. These reactions happen on the catalyst surface. They typically include adsorption of reactants, activation on the surface, reaction of the adsorbed molecules, and desorption of the products.

The nickel-catalyzed reaction of ethene and hydrogen to form ethane shows this surface process. Hydrogen first adsorbs on nickel, and the H-H bond breaks to form nickel-hydrogen bonds. Ethene also adsorbs as its carbon-carbon pi bond breaks and nickel-carbon bonds form. Hydrogen atoms then move across the surface and make new carbon-hydrogen bonds, and the ethane product desorbs from the nickel surface.

Heterogeneous catalysts are important in industry. They help make ammonia, nitric acid, sulfuric acid, and methanol. They are also used in catalytic converters in most gasoline-powered cars.

Catalyst Action in Reaction Rates

reaction rate

Measuring Reaction Rates

Measuring reaction rates shows how fast reactants are used up or products are formed over time. The rate of reaction is the change in the amount of a reactant or product per unit time. Because of that, scientists measure how a property changes as the reaction proceeds and connect that change to reactant or product amounts. For reactions that make or use a gas, the rate can be followed by changes in volume or pressure. A rate expression is the mathematical way to write how concentration changes...

measuring reaction rates

Tracking Reaction Kinetics with Light and Pressure

Reaction kinetics can be tracked with polarimetry, spectrometry, and pressure measurements. These methods let scientists follow a reaction without disturbing the sample. They also help determine how reactant or product concentrations change over time. Polarimetry is used for optically active substances. These substances rotate the plane of polarized light, which is called optical rotation. The effect comes from molecular structure. Normal monochromatic light is unpolarized, but after it passes...

concentration and rate law

Reaction Order from Concentration

Reaction order from concentration shows how reactant amounts affect reaction rate. Rate laws, also called differential rate laws or rate equations, are mathematical expressions that connect reaction rate with the concentrations of reactants. For a generic reaction a A + b B → products, the rate law can be written using the reactant concentrations [A] and [B] and a rate constant k. In a rate law, k is the rate constant for one specific reaction at one specific temperature. The exponents m and n...

determining order of reaction

Finding Rate Law from Initial Rates

Rate laws connect the speed of a chemical reaction to the concentration of its reactants. The rate constant, k, and the reaction orders are not taken from the chemical equation. They are found experimentally by watching how the rate changes when the reactant concentrations change. One common way to do this is the method of initial rates. In this method, several trials are run with different starting concentrations. The measured rates are then compared to determine the reaction orders and,...

the integrated rate law: the dependence of concentration on time

the-integrated-rate-law-the-dependence-of-concentration-on-time

Reading Reaction Progress with Integrated Laws

Integrated rate laws connect reaction concentration to time. They help show how much reactant or product is present after a certain period. They can also help estimate how long a reaction must run to reach a given extent. A common use is finding how long radioactive material must be stored before its radioactivity drops to a safe level. These equations come from the differential rate law after it is integrated with respect to time. For a first-order reaction, where rate = k[A], the integrated...

half-life of a reaction

Reaction Half-Life in Kinetics

Reaction half-life is the time needed for half of a reactant to be consumed. After each half-life, half of the remaining reactant is used up. A hydrogen peroxide decomposition example shows this pattern clearly. The concentration drops from 1.000 M to 0.500 M in the first 6.00 hours, then to 0.250 M in the next 6.00 hours, and then to 0.125 M in the third period. Each later 6.00-hour interval removes half of what is left. For first-order reactions, the half-life does not depend on the reactant...

temperature dependence on reaction rate

Collision Theory and Reaction Speed

Collision theory explains why reaction speed depends on how particles collide. Atoms, molecules, or ions must come close together before they can react. The theory says the reaction rate depends on the collision rate, the orientation of the colliding species, and whether the collision has enough energy for bonds to change. A gas-phase reaction between carbon monoxide and oxygen shows why orientation matters. The molecules can collide in more than one way. If the oxygen side of carbon monoxide...

arrhenius plots

Determining Activation Energy from Temperature

The Arrhenius equation links activation energy and the rate constant, k, for chemical reactions. It is written as k = Ae−Ea/RT. In this equation, R is the ideal gas constant with a value of 8.314 J/mol·K, T is the temperature on the kelvin scale, Ea is the activation energy in J/mole, e is the constant 2.7183, and A is the frequency factor. The frequency factor depends on collision frequency and the orientation of reacting molecules. Experimental kinetic data can be used to find the activation...

reaction mechanisms

Elementary Steps in Reaction Mechanisms

Chemical reactions can happen in steps, and a balanced equation does not show the full path at the molecular level. A reaction mechanism, also called a reaction path, gives the step-by-step process that explains how reactants become products. The decomposition of ozone is one example of a reaction that can be described by a sequence of steps. Each step in a mechanism is an elementary reaction. These elementary reactions happen in order, and when they are added together, they give the balanced...

rate-determining steps

Reaction Bottlenecks in Chemical Kinetics

Reaction bottlenecks help explain rate-determining steps in multistep reaction mechanisms. In a mechanism with several elementary steps, one step is often much slower than the others. That slowest step is called the rate-limiting step, or rate-determining step. A reaction cannot move faster than its slowest step, so this step controls the overall reaction rate. The idea is like traffic on a four-lane freeway with one lane closed. Cars can only move as fast as the bottleneck allows. In the same...

catalysis

Catalysts change the rate of a chemical reaction by giving it a faster path. A catalyst increases reaction rate without being consumed during the process. Its effect is often explained with reaction mechanisms and energy diagrams. For an endothermic reaction, the reactants and products start and end at the same energies in both cases. The uncatalyzed path is a one-step mechanism with one transition state. The catalyzed path follows a different mechanism with two transition states and a lower...

enzymes

Enzyme Action and Inhibition

Enzymes are biological catalysts that speed up many reactions in living organisms. They help control cellular metabolism by lowering the activation energy needed for biochemical reactions. When activation energy drops, reaction rates can increase. Enzyme problems can also lead to serious disease. A genetic abnormality that causes G6PD, or glucose-6-phosphate dehydrogenase, deficiency can disrupt the pathway that supplies NADPH to cells. In red blood cells, this can reduce glutathione and...

key terms and concepts

Explore how catalysts speed up reactions by lowering activation energy, with clear examples of homogeneous and heterogeneous catalysis for high school chemistry.

Catalyst Action in Reaction Rates | JoVE K12

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Pennsylvania State Academic Standards

Physical Science

Chemical Reactions

3.2.9-12.D

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Ohio’s Learning Standards and Model Curriculum

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New York State Science Learning Standards

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Catalysts in Chemical Reactions

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Alpha (&#945;) decay is the ...

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Nuclear Binding Energy

The difference between the calculated and experimentally measured masses is known as the mass defect of the atom. In the case of helium-4, the mass defect ...

Radioactive Decay and Radiometric Dating

Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

Nuclear Fission

Many heavier elements with smaller binding energies per nucleon can decompose into more stable elements that have intermediate mass numbers and larger ...

Nuclear Power

Controlled nuclear fission reactions are used to generate electricity. Any nuclear reactor that produces power via the fission of uranium or plutonium by ...

Nuclear Fusion

The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

Nuclear Transmutation

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

PS.Chm.1.2

Atomic Orbitals

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

electron-configuration-of-multielectron-atoms

Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

Use models to explain how electrons are distributed in atoms.

PS.Chm.1.3

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

The identity of a substance is defined not only by the types of atoms or ions it contains but by the quantity of each type of atom or ion. For example, ...

Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

trends-in-lattice-energy-ion-size-and-charge

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

bond-polarity-dipole-moment-and-percent-ionic-character

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

lewis-structures-of-molecular-compounds-and-polyatomic-ions

Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

molecular-comparison-of-gases-liquids-and-solids

Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

PS.Chm.3.2

Analyze the structure of atoms and isotopes.

Catalyst Action in Reaction Rates

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