Name: how reactant concentration sets reaction rate
Uploaded: 2025-05-22T09:05:33.000Z
Duration: 2 min 33 s
Channel: JoVE

K12 Standards

Florida Department of Education

High School

Physical Science

SC.912.P.12

SC.912.P.12.12

Rate Law and Reaction Order

Herhangi bir reaksiyon için, reaksiyon hızı ile reaktan konsantrasyonları arasındaki ilişki, bir hız yasası veya hız denklemi kullanılarak matematiksel olarak ifade edilebilir. 
Bir oran yasasında, 'k' orantılılık sabiti veya hız sabitidir ve 'n', değeri genellikle bir tamsayı olan tek bir reaktana göre reaksiyon sırasıdır. Çoklu reaktan reaksiyonları için hız yasalarında, genel reaksiyon sırası, tüm reaktan siparişlerinin toplamıdır.
Her reaktan için reaksiyon hızı, hız sabiti, konsantrasyon ve reaksiyon sırasının tümü deneysel olarak belirlenir.
Bireysel reaktan emirleri genellikle 0, 1 veya 2 değerlerini alır ve genel reaksiyon sırasına bağlı olarak, kimyasal reaksiyonlar sıfır dereceden, birinci dereceden veya ikinci dereceden reaksiyonlar olarak kategorize edilebilir.
Reaksiyon hızının süresi boyunca sabit kaldığı tek reaktan veya tek başına olmayan bir kimyasal reaksiyon, sıfır dereceden bir reaksiyondur. Sıfır dereceli bir reaksiyondaki reaktan sırası sıfırdır ve reaktan konsantrasyonu sıfırıncı kuvvete yükseltilir.
Sıfırıncı kuvvete yükseltilen herhangi bir sayının değeri bir olduğundan, sıfır dereceli bir reaksiyonun reaksiyon hızı, hız sabitine eşittir ve dolayısıyla reaktan konsantrasyonundan bağımsızdır.
Reaksiyon hızının reaktantın 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 kuvvete yükseltilir.
Birin kuvvetine yükseltilen herhangi bir sayının değeri aynı kaldığından, birinci dereceden bir reaksiyonun reaksiyon hızı doğrudan reaktan konsantrasyonuna bağlıdır. Reaktan konsantrasyonu azaldıkça, reaksiyon hızı doğrusal bir şekilde orantılı olarak azalır.
Reaksiyon hızının reaktan konsantrasyonunun karesine bağlı olduğu tek moleküllü bir kimyasal reaksiyon, ikinci dereceden bir reaksiyondur. Reaktan konsantrasyonu azaldıkça, reaksiyon hızı ikinci dereceden bir şekilde katlanarak azalır.

hız yasası ve reaksiyon sırası

<div>
 Bir reaksiyonun hızı reaktanların konsantrasyonundan etkilenir. Hız yasaları (diferansiyel hız yasaları) veya hız denklemleri, bir kimyasal reaksiyonun hızı ile reaktanların konsantrasyonu arasındaki ilişkiyi tanımlayan matematiksel ifadelerdir.
 
 Örneğin, a ve b'nin stokiyometrik katsayılar olduğu genel bir aA + bB ⟶ çarpımı reaksiyonunda hız yasası şu şekilde yazılabilir:
 
 hız = k[A]^m[B]^n

 [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 dereceleridir ve kesirler, negatif değerler veya sıfır olabilmelerine rağmen tipik olarak pozitif tam sayılardır.
 

 Hız sabiti k ve reaksiyon dereceleri m ve n, reaktanların konsantrasyonları değiştikçe reaksiyon hızının nasıl değiştiğinin gözlemlenmesi ile deneysel olarak belirlenir. Hız sabiti k, reaktan konsantrasyonlarından bağımsızdır ancak sıcaklığa göre değişir.
 

 Hız yasasındaki reaksiyon dereceleri, hızın reaktan konsantrasyonlarına matematiksel bağımlılığını tanımlar. Genel hız yasasına göre (hız = k[A]^m[B]^n), reaksiyon A'ya göre m'inci dereceden ve B'ye göre n'inci derecedendir. Örneğin, eğer m = 1 ve n = 2 ise, reaksiyon A'da birinci dereceden ve B'de ikinci derecedendir. Genel reaksiyon sırası basitçe her reaktanın derecelerinin toplamıdır. Buradaki örnek hız yasası için reaksiyon genel olarak üçüncü derecedendir (1 + 2 = 3).
 

 Hız yasalarının belirlenmesine yönelik yaygın bir deneysel yaklaşım, başlangıç ​​hızları yöntemidir. Bu yöntem, farklı başlangıç ​​reaktan konsantrasyonları kullanılarak gerçekleştirilen çoklu deneysel denemeler için reaksiyon hızlarının ölçülmesini içerir. Bu denemeler için ölçülen oranların karşılaştırılması, reaksiyon sıralarının ve ardından hız sabitinin belirlenmesine olanak tanır ve bunlar birlikte bir hız yasası formüle etmek için kullanılır.
 
 Hız yasaları bazı reaktanlar için kesirli dereceler sergileyebilir ve bazen bir reaktanın konsantrasyonundaki bir artış reaksiyon hızında bir azalmaya neden olduğunda negatif reaksiyon dereceleri gözlemlenir. Hız yasalarının yalnızca deneyle belirlendiğini ve reaksiyon stokiyometrisi ile güvenilir bir şekilde tahmin edilemediğini belirtmek önemlidir.
 
 Reaksiyon sırası, reaksiyon hızı ile reaktanların veya ürünlerin konsantrasyonu arasındaki ilişkiyi belirler.
 

 <ul style="list-style-type: disc; display: flex; flex-direction: column; gap: 10px; padding: 0 0 0 40px;">
 <li>Sıfır dereceli bir reaksiyonda, reaktanların konsantrasyonunun reaksiyon hızı üzerinde herhangi bir etkisi yoktur ve reaksiyon boyunca sabit kalır.
 </li>
 <li>Birinci dereceden bir reaksiyonda reaksiyon hızı, reaktan konsantrasyonundaki değişiklikle doğrudan ve doğrusal olarak orantılıdır. Reaktif konsantrasyonu azaldıkça reaksiyon hızı da orantılı olarak azalır.
 </li>
 <li>İkinci dereceden veya daha yüksek dereceden reaksiyonlarda reaksiyon hızı, reaktanların üstel değeriyle orantılıdır. Bu nedenle reaksiyon ilerledikçe ve reaktanların konsantrasyonu azaldıkça reaksiyon hızı katlanarak azalır.
 </li>
 </ul>
 Bu metin ABC’den uyarlanmıştır<a href="https://openstax.org/books/chemistry-2e/pages/12-3-rate-laws#57033">Openstax, Chemistry 2e, Section 12.3: Rate Laws</a>.

</div>

Hız Yasası ve Reaksiyon Sırası

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

Education

JoVE Core

Organic Chemistry

Organik Kimya

Unit 1

Ünite 1

Thermodynamics and Chemical Kinetics

Termodinamik ve Kimyasal Kinetik

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

how reactant concentration sets reaction rate

Reaction rate depends on reactant concentration, and rate laws show that relationship with a mathematical equation. A rate law, also called a differential rate law or rate equation, links the rate of a chemical reaction to the concentrations of its reactants.

For a generic reaction, a A + b B  products, the rate law can be written as rate = k [A]^m [B]^n. Here, [A] and [B] are the molar concentrations of the reactants. The constant k is the rate constant, and it is specific to one reaction at a specific temperature.

The exponents m and n are the reaction orders. They are usually positive integers, but they can also be fractions, negative values, or zero. 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 separate orders, so this example is third order overall.

Rate law values are found by experiment, not by stoichiometry. Scientists change the initial reactant concentrations in several trials and measure the reaction rate. This method, called the method of initial rates, helps determine the reaction orders and then the rate constant.

Some reactions show zero-order behavior. In a zero-order reaction, changes in reactant concentration do not change the rate, so the rate stays constant. In a first-order reaction, the rate changes in direct proportion to the reactant concentration. In second-order and higher-order reactions, the rate depends on the concentration raised to an exponent, so the rate drops more sharply as reactants are used up.

Rate laws can also show fractional orders, and some can even show negative orders. A negative order means that increasing one reactant can decrease the reaction rate. These patterns are useful for describing how reaction rate changes in real experiments. They are not reliably predicted from the reaction equation alone, so the rate law must be determined experimentally.

How Reactant Concentration Sets Reaction Rate

how-reactant-concentration-sets-reaction-rate

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rate law and reaction order

Reaction rate depends on reactant concentration, and rate laws show that relationship with a mathematical equation. A rate law, also called a differential rate law or rate equation, links the rate of a chemical reaction to the concentrations of its reactants. For a generic reaction, a A + b B  products, the rate law can be written as rate = k [A]^m [B]^n. Here, [A] and [B] are the molar concentrations of the reactants. The constant k is the rate constant, and it is specific to one reaction at...

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key terms and concepts

Learn how rate laws connect reactant concentration to reaction speed, how reaction orders work, and how the method of initial rates is used to find them.

How Reactant Concentration Sets Reaction Rate | JoVE K12

organic chemistry

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How Reactant Concentration Sets Reaction Rate

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