Learn Chemical Kinetics

Name: Learn Chemical Kinetics
Rating: 3.5 (1 reviews)

Rates of Rection

Created byVinay Arya

Last updated 5/2022

English

What you'll learn

The students will get a wide picture of rate of reaction
The students will learn about slow and fast reactions.
The students will have a deep knowledge about the reaction parameters.
The students will know about the importance of fast reactions in daily life.

Course content

1 section • 18 lectures • 3h 32m total length

4.1. Contents to Chemical Kinetics12:48
Explore the contents of chemical kinetics, including rate of reaction, rate laws, order, integrated rate laws, activation energy, Arrhenius equation, catalysts, and collision theory.
4.2. Chemical Kinetics - Introduction18:15
Explore chemical kinetics, studying the rate of reaction and its mechanism, and understand why reactions are very fast, very slow, or moderately fast using concentration changes.
4.3. Rate of a Chemical Reaction16:30
Define the rate of a chemical reaction from changes in reactant and product concentrations. Apply stoichiometric coefficients, sign conventions, and unit conversions, including partial pressures via the ideal gas equation.
4.4. Average Rate and Instantaneous Rate10:35
Explore the concepts of average rate and instantaneous rate in chemical kinetics, define rate as the change in concentration over time, and illustrate experimental determination with concentration-time graphs.
4.5. Factors Influencing Rate of a Reaction11:07
Explore how concentration, temperature, the nature of reactants, catalysts, and radiation influence reaction rates, and understand rate laws, rate expressions, and rate constants that quantify these effects.
4.6. Dependence of Rate on Concentration16:00
Learn how reaction rate depends on concentration through rate laws and rate expressions, and how initial-rate experiments determine the rate constant and reaction order.
4.7. Molecularity of a Reaction13:00
Explore molecularity in chemical reactions, distinguishing unimolecular, bimolecular, and termolecular steps, and connect collision theory to rate laws and rate-determining steps.
4.8. Order of Reaction11:58
Learn how the order of reaction, defined as the sum of exponents in the rate law, is determined experimentally and includes zero, first, second, fractional, and pseudo orders.
4.9. Integrated Rate Equations12:23
Explore how integrated rate equations connect concentration versus time to determine reaction order and rate constants, with zero-, first-, and second-order cases, half-life, and graphical methods.
4.10.Pseudo First Order Reaction7:59
Learn how pseudo first order reactions arise when one reactant is in large excess, making the rate appear first order while the true order differs; explore examples and implications.
4.11. Methods for Calculating the Value of Rate Constant10:35
Explore methods for calculating the rate constant in chemical kinetics, using gas-phase first-order reactions with total and partial pressures and a numerical example to determine k.
4.12. Half Life of a Reaction13:26
Explore the concept of half life in chemical kinetics, including zeroth and first-order cases, with carbon-14 dating as a key application, and learn to calculate t1/2 from rate constants.
4.13. Temperature Dependence of the Rate of a Reaction8:51
Discover how temperature governs the rate of chemical reactions, with examples of faster rates at higher temperatures. Explain this dependence using the Arrhenius equation and activation energy.
4.14. Activation Energy12:44
Explore activation energy and the energy barrier that must be crossed for reactants to form products, via collisions, transition states, and the activated complex in chemical kinetics.
4.15. Arrhenius Equation10:24
Link temperature to reaction rate using the Arrhenius equation, derive activation energy and frequency factor, and interpret log k versus 1/T with graphical and two-point methods.
4.16. Effect of Catalyst9:42
Show how a catalyst lowers activation energy by providing an alternative reaction pathway and absorbing nitrogen and hydrogen on its surface to increase the rate of reaction without changing equilibrium.
4.17. Collision theory of Chemical Reactions8:35
Explore the collision theory of chemical reactions, linking collision frequency, activation energy, and orientation to reaction rates, and see how the Arrhenius equation and energy barriers shape kinetics.
4.18. Factor Affecting Rate of Reaction7:51
Explore factors in chemical kinetics affecting the rate of reaction, including temperature, concentration, pressure, and catalysts; and how state, size, and activation energy influence speed.

Requirements

The child should have a clear concepts of types of reactions.

Description

A chemical change involves changing reactants to products. A balanced equation is an essential quantitative tool for calculating product yields from reactant amounts, but it tells us nothing about three dynamic aspects of the reaction, which are essential to understanding chemical change. For any chemical reaction, chemists try to find out

1. How fast is the reaction proceeding at a given moment?

2. What will be the reactant and product concentrations when the reaction is complete?

3. Will the reaction proceed by itself and release energy, or will it require energy to proceed?

This lecture addresses the first of these questions and focuses on the field of kinetics, which deals with the speed of a reaction and its mechanism, the stepwise changes that reactants undergo in their conversion to products.

The extent to which a reaction will proceed can be determined from chemical equilibrium whereas the feasibility of a chemical reaction can be predicted by thermodynamics (DG < 0). The knowledge of free energy change of a reaction however gives us no idea about the rate and the factors controlling the rate of a reaction.

For example,

Why do some reactions occur slowly while others seem to take place

instantaneously?

How does chemist's measure, compare and express the rates at which chemical reactions occur?

Can chemists predict and control the rate of a chemical reaction?

How quickly a chemical reaction occurs is a crucial factor in how the reaction affects its surroundings. Therefore, knowing the rate of a chemical reaction is integral to understanding the reaction. For example,

How quickly a medicine acts or blood clots can make the difference between life and death.

How long it takes for cement to harden or polyethylene to form can make the difference between profit and loss.

All these questions can be answered by the branch of chemistry known as

Chemical kinetics.

Who this course is for:

For the Beginners and students of twelfth standard.