Name: reaction order from concentration
Uploaded: 2020-09-24T15:06:50.000Z
Duration: 3 min 3 s
Channel: JoVE

K12 Standards

Texas Essential Knowledge and Skills

High School

Chemistry and Physics

IPC.7

IPC.7.F

Concentration and Rate Law

Bir reaksiyonun hızı genellikle reaktan konsantrasyonlarına bağlıdır. Herhangi bir reaksiyon için, reaksiyon hızı ile reaktan konsantrasyonları arasındaki ilişki, bir hız yasası veya hız denklemi kullanılarak matematiksel olarak ifade edilebilir. Hız yasasında, k orantılılık sabiti veya hız sabitidir ve n, değeri genellikle bir tam sayı olan tek bir reaktant ile ilgili olarak reaksiyon sırasıdır.Çok reaktantlı reaksiyonlar için hız kanunlarında, genel reaksiyon sırası, tüm reaktan siparişlerinin toplamıdır. Her reaktan için, reaksiyon hızı, hız sabiti, konsantrasyon ve reaksiyon sırası deneysel olarak belirlenir. Oran yasası, tüm bu parametreler arasındaki ilişkiyi ifade eder.Ayrı ayrı reaktan sıraları genellikle 0, 1 veya 2 değerlerini alır ve genel reaksiyon sırasına göre kimyasal reaksiyonlar sıfır dereceli, birinci dereceden veya ikinci dereceden reaksiyonlar olarak kategorize edilebilir. Reaksiyon hızının süresi boyunca sabit kaldığı tek reaktanlı veya tek moleküllü kimyasal reaksiyon sıfır dereceli bir reaksiyondur. Sıfır dereceli bir reaksiyondaki reaktan sırası sıfırdır ve hız kanununa göre reaktan konsantrasyonu sıfırıncı güce yükseltilir.Sıfırıncı güce yükseltilen herhangi bir sayının değeri bir olduğundan, sıfır dereceli bir reaksiyonun reaksiyon hızı, hız sabitine eşittir ve dolayısıyla, reaktan konsantrasyonundan bağımsızdır. Bu nedenle, sıfır dereceli bir reaksiyonda, reaktantın konsantrasyonu azalsa bile reaksiyon hızı yavaşlamaz. Reaksiyon hızının reaktanın konsantrasyonu ile doğru orantılı olduğu tek moleküllü bir kimyasal reaksiyon, birinci dereceden bir reaksiyondur.Birinci dereceden bir reaksiyon için reaktan sırası birdir ve hız yasasına göre reaktantın konsantrasyonu birinci güce yükseltilir. Birinin gücüne yükseltilen herhangi bir sayının değeri aynı kaldığından, birinci dereceden bir reaksiyonun reaksiyon hızı, doğrudan reaktan konsantrasyonuna bağlıdır. Reaktan konsantrasyonu azaldıkça, reaksiyon hızı orantılı olarak doğrusal bir şekilde azalır.Reaksiyon hızının reaktant konsantrasyonunun karesine bağlı olduğu tek moleküllü bir kimyasal reaksiyon, ikinci dereceden bir reaksiyondur. Reaktan sırası ikidir ve reaktan konsantrasyonu ikinci güce yükseltilir. Buna göre, ikinci dereceden bir reaksiyondaki reaksiyon hızı, doğrudan reaktan konsantrasyonunun karesine bağlıdır.Reaktan konsantrasyonu azaldıkça, reaksiyon hızı ikinci dereceden bir şekilde üssel olarak azalır.

hız yasasının konsantre hali

Bir reaksiyonun hızı, reaktanların konsantrasyonlarından etkilenir. Hız yasaları (diferansiyel hız yasaları) veya hız denklemleri, bir kimyasal reaksiyonun hızı ile reaktanlarının konsantrasyonu arasındaki ilişkiyi tanımlayan matematiksel ifadelerdir.
 
 Örneğin, a ve b'nin stokiyometrik katsayılar olduğu genel bir reaksiyon olan aA + bB ⟶ Ürünler; oran yasası şu şekilde yazılabilir:
 
  <img alt="Eq1" src="/files/ftp_upload/11375/11375_Equation_1.png" style="height: 50px;" />
 
 [A] ve [B], reaktanların molar konsantrasyonlarını temsil eder ve k, belirli bir sıcaklıkta belirli bir reaksiyon için spesifik olan hız sabitidir.
 
 m ve n üsleri reaksiyon sıralarıdır ve genellikle pozitif tamsayılardır, ancak kesirler, negatif veya sıfır da olabilirler.
 
 Hız sabiti k ve reaksiyon sıraları m ve n, reaktanların konsantrasyonları değiştikçe bir reaksiyon hızının nasıl değiştiği gözlemlenerek deneysel olarak belirlenir. Hız sabiti k, reaktan konsantrasyonlarından bağımsızdır, ancak sıcaklığa göre değişir.
 
 Bir hız yasasındaki reaksiyon sıraları, hızın reaktan konsantrasyonlarına matematiksel bağımlılığını tanımlar. Genel oran yasasına (hız = k[A]m[B]n) bakıldığında, reaksiyon B'ye göre A ve n mertebesine göre m mertebesidir.Örneğin, m = 1 ve n = 2 ise, reaksiyon A'da birinci mertebedir ve ikinci B. Genel reaksiyon sırası, her reaktan için sıraların toplamıdır. Buradaki örnek oran yasası için, reaksiyon genel olarak üçüncü derecedir (1 + 2 = 3).
 
 Oran yasalarının belirlenmesine yönelik yaygın bir deneysel yaklaşım, başlangıç oranlarının yöntemidir. Bu yöntem, farklı başlangıç reaktan konsantrasyonları kullanılarak gerçekleştirilen çoklu deneysel denemeler için reaksiyon hızlarının ölçülmesini içerir. Bu denemeler için ölçülen hızların karşılaştırılması, birlikte bir oran yasasını formüle etmek için kullanılan reaksiyon sıralarının ve ardından hız sabitinin belirlenmesine izin verir.
 
 Hız yasaları bazı reaktanlar için kesirli sıralar gösterebilir ve bazen bir reaktantın konsantrasyonundaki bir artış reaksiyon hızında bir düşüşe neden olduğunda negatif reaksiyon sıraları gözlemlenir. Hız yasalarının yalnızca deneyle belirlendiğini ve reaksiyon stokiyometrisi ile güvenilir bir şekilde tahmin edilmediğini unutmamak önemlidir.
 
 Reaksiyon sırası, reaksiyon hızı ile reaktanların veya ürünlerin konsantrasyonu arasındaki ilişkiyi belirler.
 
 • Sıfır dereceli bir reaksiyonda, reaktanların konsantrasyonu, reaksiyon boyunca sabit kalan reaksiyon hızı üzerinde herhangi bir etkiye sahip değildir. 
 • Birinci dereceden bir reaksiyonda, reaksiyon hızı, reaktan konsantrasyonundaki değişiklikle doğrudan ve doğrusal orantılıdır. Reaktan konsantrasyonu azaldıkça, reaksiyon hızı da orantılı olarak azalır. 
 • İkinci dereceden veya daha yüksek dereceden reaksiyonlarda, reaksiyon hızı, reaktanların üstel değeriyle orantılıdır. Bu nedenle, reaksiyon ilerledikçe ve reaktanların konsantrasyonu azaldıkça, reaksiyon hızı üssel olarak azalır.
 
 Bu metin bu kaynaktan uyarlanmıştır <a href="https://openstax.org/books/chemistry-2e/pages/12-3-rate-laws#57033">Openstax, Chemistry 2e, Section 12.3: Rate Laws</a>.

Hız Yasasının Konsantre Hali

Bir reaksiyonun hızı, reaktanların konsantrasyonlarından etkilenir. Oran yasaları (diferansiyel oran yasaları) veya oran denklemleri matematiksel ifadelerdir ...

Education

JoVE Core

Chemistry

Kimya

Chemical Kinetics

Kimyasal Kinetik

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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 are the reaction orders. They are usually positive integers, but they can also be fractions, negative numbers, or zero. The values of k, m, and n are found experimentally by measuring how the rate changes when reactant concentrations change.

The rate constant does not depend on the reactant concentrations, but it can change with temperature. The reaction orders show the mathematical link between concentration and rate. In the expression rate = k [A]m [B]n, the reaction is m order with respect to A and n order with respect to B. For example, if m = 1 and n = 2, the reaction is first order in A and second order in B.

The overall reaction order is the sum of the orders for each reactant. In the example above, the reaction is third order overall because 1 + 2 = 3. A common way to find a rate law is the method of initial rates. In this method, reaction rates are measured in several trials that start with different initial reactant concentrations. Comparing those rates makes it possible to find the reaction orders and then the rate constant.

Rate laws can also include fractional orders. In some cases, a reactant may have a negative order. That means increasing its concentration can lower the reaction rate. Rate laws are determined by experiment only, and they cannot be reliably predicted from reaction stoichiometry. The reaction order also describes how the rate changes as reactant or product concentration changes.

A zero-order reaction has a rate that does not change with reactant concentration. The rate stays constant throughout the reaction. In a first-order reaction, the rate is directly proportional to the change in reactant concentration. As the reactant concentration drops, the rate drops by the same proportion. In second-order or higher-order reactions, the rate depends on the reactants raised to an exponent. As the reaction continues and reactant concentration decreases, the rate falls exponentially.

Reaction Order from Concentration

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concentration and rate law

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...

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key terms and concepts

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Reaction Order from Concentration | JoVE K12

chemistry

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Matter and its Interactions

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Physical Science

Chemical Reactions

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New York State Science Learning Standards

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Reaction Order from Concentration

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