Name: arrhenius equation in reaction speed
Uploaded: 2023-04-30T18:28:32.000Z
Duration: 2 min 28 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-5

effect-of-temperature-change-on-reaction-rate

Effect of Temperature Change on Reaction Rate

חוק קצב התגובה מגדיר את הקשר בין ריכוז מגיב לבין קצב התגובה במונחים של קבוע קצב, 'k'.
קבוע הקצב מתאר את הקשר בין טמפרטורה ופרמטרים קינטיים הקשורים להתנגשות, אוריינטציה ואנרגיית שפעול של מולקולות מגיבות באמצעות משוואת ארניוס. A הוא קבוע הנקרא גורם ארניוס או גורם תדירות. 'e' הוא גורם מעריכי המשלב אנרגיית שפעול הנמדדת בג'אול לשומה, קבוע הגז והטמפרטורה בקלבין.
ניתן להסביר את התלות בטמפרטורה של הפרמטרים באמצעות מודל ההתנגשות, הקובע כי מולקולות מגיבות צריכות להתנגש באנרגיה מספקת בכיוון הנכון כדי ליזום תגובה כימית.
גורם התדר מורכב משני מרכיבים – תדירות ההתנגשות וגורם הכיוון. תדירות ההתנגשות היא מספר ההתנגשויות המולקולריות ליחידת זמן, ואילו גורם האוריינטציה מתאר את ההסתברות להתנגשויות עם אוריינטציה חיובית.
ובכל זאת, רק חלק קטן מההתנגשויות מוביל לתגובה. הסיבה לכך היא שהמולקולות המגיבות צריכות להתגבר על מחסום אנרגיה, שנקרא אנרגיית שפעול, כדי להפוך לתוצרים.
רק למולקולות המתנגשות באנרגיה קינטית מספקת תהיה מספיק אנרגיה פוטנציאלית כדי לכופף, למתוח או לשבור קשרים כדי להפוך למתווך בעל אנרגיה גבוהה שנקרא מצב המעבר, או המכלול המופעל. הקומפלקס המופעל קצר החיים והבלתי יציב מאבד אנרגיה ליצירת תוצרים יציבים, שהאנרגיה הכוללת שלהם נמוכה מזו של המגיבים.
הגורם המעריכי במשוואת ארניוס מייצג את שבריר ההתנגשויות המוצלחות הנובעות מתוצרים. עלייה בטמפרטורה משפיעה הן על גורם התדירות והן על הגורם המעריכי.
בטמפרטורות גבוהות, מולקולות נעות מהר יותר, בעוצמה רבה יותר ובאנרגיות תרמיות גבוהות יותר, מה שמוביל להתנגשויות טובות יותר.
עבור רוב התגובות, עליית טמפרטורה גורמת לתדירות גבוהה יותר ולגורמים מעריכיים, מה שמוביל לעלייה בקבוע הקצב, וכתוצאה מכך מתורגם לקצב תגובה מואץ.

﻿השפעת שינוי הטמפרטורה על קצב התגובה

<div style="direction:rtl"> משוואת ארניוס, <img alt="Figure1" src="/files/ftp_upload/11698/11698_Equation1.svg" style="text-align: center; height: 30px;"> מקשרת את אנרגיית השפעול וקבוע הקצב, k, עבור תגובות כימיות רבות. במשוואה זו, R הוא קבוע הגז האידיאלי, בעל ערך 8.314 J/mol·K, T הוא הטמפרטורה בקלווין, E_a הוא אנרגיית ההפעלה בג'אול למול, e הוא הקבוע 2.7183, ו-A הוא קבוע נקרא גורם התדירות, הקשור לתדירות ההתנגשויות ולכיוון המולקולות המגיבות. גורם התדירות, A, משקף עד כמה תנאי התגובה מעדיפים התנגשויות בכיוון נכון בין מולקולות מגיבים. סבירות מוגברת להתנגשויות מכוונות ביעילות גורמת לערכים גדולים יותר עבור A וקצבי תגובה מהירים יותר. המונח האקספוננציאלי, e −Eₐ/RT , מתאר את השפעת אנרגיית השפעול על קצב התגובה. על פי התיאוריה המולקולרית הקינטית, טמפרטורת החומר היא מדד לאנרגיה הקינטית הממוצעת של האטומים או המולקולות המרכיבות אותו - אנרגיית שפעול נמוכה יותר מביאה לחלק משמעותי יותר של מולקולות עם אנרגיה מספקת ולתגובה מהירה יותר. המונח האקספוננציאלי מתאר גם את השפעת הטמפרטורה על קצב התגובה. טמפרטורה גבוהה יותר מייצגת חלק גדול יותר של מולקולות בעלות מספיק אנרגיה (RT) כדי להתגבר על מחסום השפעול (E_a). זה נותן ערך גבוה יותר עבור קבוע הקצב וקצב תגובה מהיר יותר בהתאם. האנרגיה המינימלית הדרושה ליצירת תוצר במהלך התנגשות בין מגיבים נקראת אנרגיית השפעול (E_a). ההפרש בין אנרגיית השפעול הנדרשת והאנרגיה הקינטית שמספקות מולקולות מגיבים מתנגשות הוא גורם ראשוני המשפיע על קצב התגובה הכימית. אם אנרגיית השפעול גדולה בהרבה מהאנרגיה הקינטית הממוצעת של מולקולות, התגובה תתרחש באיטיות, שכן רק לכמה מולקולות הנעות במהירות תהיה מספיק אנרגיה כדי להגיב. אם אנרגיית השפעול קטנה בהרבה מהאנרגיה הקינטית הממוצעת של המולקולות, חלק גדול של מולקולות יהיה אנרגטי מספיק, והתגובה תתקדם בקצב. דיאגרמות תגובה נמצאים בשימוש נרחב בקינטיקה כימית כדי להמחיש תכונות שונות של התגובה הנחקרת. זה מראה כיצד האנרגיה של מערכת כימית משתנה כשהיא עוברת תגובה, והופכת מגיבים למוצרים. הטקסט הזה מותאם מ <a href="https://openstax.org/books/chemistry-2e/pages/12-5-collision-theory"> Openstax, Chemistry 2e, Section 12.5: Collision Theory. </a> </div>

משוואת ארניוס,

מתייחס לאנרגיית ההפעלה וקבוע הקצב, k, עבור תגובות כימיות רבות.
במשוואה זו, R הוא הגז האידיאלי ...

Education

JoVE Core

Organic Chemistry

כימיה אורגנית

Unit 1

יחידה 1

Thermodynamics and Chemical Kinetics

תרמודינמיקה וקינטיקה כימית

KEY TERMS AND CONCEPTS

מונחים ומושגים מרכזיים

arrhenius equation in reaction speed

The Arrhenius equation connects activation energy, temperature, and the rate constant, k, for many chemical reactions. It helps explain why some reactions move slowly while others happen faster.

In this equation, R is the ideal gas constant, with a value of 8.314 J/mol·K. T is the temperature in kelvin, Ea is the activation energy in joules per mole, e is the constant 2.7183, and A is the frequency factor.

The frequency factor, A, describes how often reacting molecules collide and how well they are oriented during those collisions. Better orientation increases the chance of effective collisions. That leads to larger A values and faster reaction rates.

The exponential term, e−Ea/RT, shows how activation energy affects the reaction rate. Kinetic molecular theory says that temperature measures the average kinetic energy of atoms or molecules. When activation energy is lower, more molecules have enough energy to react, and the reaction is faster.

The same exponential term also shows the effect of temperature. At higher temperature, a larger fraction of molecules has enough energy, RT, to get over the activation barrier, Ea. This increases the rate constant and speeds up the reaction.

Activation energy is the minimum energy needed to form products during a collision between reactants. If Ea is much larger than the average kinetic energy of the molecules, only a few fast-moving molecules can react, so the reaction is slow. If Ea is much smaller than the average kinetic energy, many molecules can react, so the reaction proceeds quickly.

Reaction diagrams are often used in chemical kinetics to show how a system’s energy changes as reactants turn into products. They help visualize the energy barrier and the path from reactants to products. This text is adapted from Openstax, Chemistry 2e, Section 12.5: Collision Theory.

Arrhenius Equation in Reaction Speed

chemical reactions

Stoichiometry, Rates, and Equilibrium

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gibbs free energy and thermodynamic favorability

gibbs-free-energy-and-thermodynamic-favorability

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Temperature changes can decide whether a process is spontaneous. This idea applies to phase changes and to some chemical reactions. The key link is Gibbs free energy, which connects free energy change with enthalpy and entropy. The sign of the Gibbs free energy change, or ΔG, depends on the signs of enthalpy change (ΔH) and entropy change (ΔS), and sometimes on the absolute temperature. Because temperature is measured in kelvin, it is always a positive value. That means there are four main...

chemical and solubility equilibria

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rate law and reaction order

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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...

effect of temperature change on reaction rate

The Arrhenius equation connects activation energy, temperature, and the rate constant, k, for many chemical reactions. It helps explain why some reactions move slowly while others happen faster. In this equation, R is the ideal gas constant, with a value of 8.314 J/mol·K. T is the temperature in kelvin, Ea is the activation energy in joules per mole, e is the constant 2.7183, and A is the frequency factor. The frequency factor, A, describes how often reacting molecules collide and how well...

multi-step reactions

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Chemical reactions can happen in a sequence of steps. A balanced chemical equation shows the reactants and products, but it does not show how the reaction occurs at the molecular level. The reaction mechanism, or reaction path, gives that step-by-step detail. Each step in a mechanism is an elementary reaction. These elementary reactions happen in order, and together they add up to the balanced equation for the overall reaction. In a multistep mechanism, one step is often much slower than the...

bond dissociation energy and activation energy

bond-dissociation-energy-and-activation-energy

How Bond Strength Shapes Reaction Speed

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energy diagrams, transition states, and intermediates

energy-diagrams-transition-states-and-intermediates

Reaction Coordinate Diagrams in Chemical Reactions

Reaction coordinate diagrams show how energy changes during a chemical reaction. These free-energy graphs use the horizontal axis to show reaction progress. Points near the reactants look like the reactants, while points near the products look like the products. The peaks on the diagram represent stable structures with measurable lifetimes. Other points on the curve are unstable and cannot be isolated. The high-energy, unstable peak is called the transition state, or activated complex. At the...

predicting reaction outcomes

How Temperature Changes Reaction Rate

Reaction rate and reaction pathway are key ideas in chemical kinetics. Thermodynamics, by contrast, focuses on the state of a system. It describes the properties, behavior, and components of reactants and products. It does not describe the path of the process or the speed of the reaction. Kinetics gives information on the atomic or molecular level, while thermodynamics focuses on the energetics of the reactants and products. Thermodynamics can show what may happen in a reaction, but it does...

key terms and concepts

Explore how the Arrhenius equation links temperature, activation energy, and collision orientation to reaction speed in high school chemistry.

Arrhenius Equation in Reaction Speed | JoVE K12

organic chemistry

JoVE Core Organic Chemistry explains basic concepts of stereochemistry, reactions, and mechanisms using concise and easy-to-understand animated video lessons. Additionally, the scientist-in-action videos demonstrate the application of related concepts in classical and original research experiments performed in today's laboratories worldwide.

Minnesota Academic Standards in Science

9-12

3.2.1 9C.3.1.1.2

Florida Department of Education

Physical Science

SC.912.P.12

SC.912.P.12.12

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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 ...

Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.  Clarification Statement: Emphasis is on the idea that a chemical reaction is a system that affects the energy change.  Examples of models could include molecular-level drawings and diagrams of reactions, graphs showing the relative energies of reactants and products, and representations showing energy is conserved.

HS-PS1-4

The Arrhenius equation,

relates the activation energy and the rate constant, k, for many chemical reactions.
In this equation, R is the ideal gas ...

Apply scientific principles and evidence to provide an explanation about the effects of changing the temperature or concentration of the reacting particles on the rate at which a reaction occurs.  Clarification Statement: Student reasoning should focus on the number and energy of collisions between molecules.  Emphasis is on simple reactions in which there are only two reactants; evidence from temperature, concentration, and rate data;  and qualitative relationships between rate and temperature.

Arrhenius Equation in Reaction Speed

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