•

11 Feb 2026

•

2 pages

Easy Chemistry: Rate Equations and Fun Experiments!

Rishek M

@rishek.manta

This document covers key concepts in chemical kinetics, focusing on... Show more

$# RATES 2 $ \Leftrightarrow$ the change in $\boxed{concentration}$ of a product/reactant $ \boxed{over time}$ $\Rightarrow$ typical units a$

Page 2: Advanced Kinetics Concepts

This page delves into more advanced concepts in chemical kinetics.

Half-Life and First-Order Reactions

Definition: Half-life (t½) is the time taken for the concentration of a reactant to halve.

First-order reactions have a constant half-life, which can be used to identify them.

Calculating Rate Constants from Concentration-Time Data

Two methods are presented:

Using the half-life formula: k = ln(2) / t½
Using the gradient of a rate-concentration graph

Arrhenius Equation

Vocabulary: The Arrhenius equation relates the rate constant to temperature and activation energy.

The page provides the standard and logarithmic forms of the Arrhenius equation:

Standard form: k = Ae^ $-Ea/RT$
Logarithmic form: ln k = -Ea/RT + ln A

Methods for finding Ea (activation energy) and A $pre-exponential factor$ are outlined.

Rate Mechanisms

Definition: The rate-determining step is the slowest step in a reaction mechanism.

An important rule is presented: The rate equation includes all reactants in and before the rate-determining step.

Highlight: The number of moles of a reactant in the rate-determining step equals its order in the rate equation.

The page concludes with graphical representations of zero-order, first-order, and second-order reactions, emphasizing the importance of understanding these graphs for kinetic analysis.

$# RATES 2 $ \Leftrightarrow$ the change in $\boxed{concentration}$ of a product/reactant $ \boxed{over time}$ $\Rightarrow$ typical units a$

Page 1: Rate Equations and Experimental Analysis

This page focuses on rate equations and experimental methods for determining reaction orders.

Definition: A rate equation expresses the rate of a reaction in terms of the concentrations of reactants and a rate constant.

The page outlines a model answer structure for analyzing experiments to determine reaction orders:

Compare experiments where only one reactant concentration changes.
Observe how the rate changes with concentration changes.
Determine the order of each reactant based on these observations.

Example: If doubling [A] increases the rate by a factor of 4, the order with respect to A is 2.

The page also covers concentration-time graphs for different reaction orders:

Highlight: The shape of concentration-time graphs depends on the overall order of the reaction:

First order: exponential decay

Second order: reciprocal plot

Third order: more complex curve

Determining Rate Constants

The method for calculating rate constants is explained:

Rearrange the rate equation to solve for k.
Substitute values from one of the given experiments.

Example: For a rate equation Rate = k[A]²[B], rearrange to k = Rate / ([A]²[B]) and substitute values.

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Chemistry

•

11 Feb 2026

•

2 pages

Easy Chemistry: Rate Equations and Fun Experiments!

Rishek M

@rishek.manta

This document covers key concepts in chemical kinetics, focusing on rate equations, experimental analysis, and reaction mechanisms. It provides detailed explanations and methods for determining reaction orders, rate constants, and activation energies.

Overall Summary:

The document provides a comprehensive... Show more

$# RATES 2 $ \Leftrightarrow$ the change in $\boxed{concentration}$ of a product/reactant $ \boxed{over time}$ $\Rightarrow$ typical units a$

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Page 2: Advanced Kinetics Concepts

This page delves into more advanced concepts in chemical kinetics.

Half-Life and First-Order Reactions

Definition: Half-life (t½) is the time taken for the concentration of a reactant to halve.

First-order reactions have a constant half-life, which can be used to identify them.

Calculating Rate Constants from Concentration-Time Data

Two methods are presented:

Using the half-life formula: k = ln(2) / t½
Using the gradient of a rate-concentration graph

Arrhenius Equation

Vocabulary: The Arrhenius equation relates the rate constant to temperature and activation energy.

The page provides the standard and logarithmic forms of the Arrhenius equation:

Standard form: k = Ae^ $-Ea/RT$
Logarithmic form: ln k = -Ea/RT + ln A

Methods for finding Ea (activation energy) and A $pre-exponential factor$ are outlined.

Rate Mechanisms

Definition: The rate-determining step is the slowest step in a reaction mechanism.

An important rule is presented: The rate equation includes all reactants in and before the rate-determining step.

Highlight: The number of moles of a reactant in the rate-determining step equals its order in the rate equation.

The page concludes with graphical representations of zero-order, first-order, and second-order reactions, emphasizing the importance of understanding these graphs for kinetic analysis.

$# RATES 2 $ \Leftrightarrow$ the change in $\boxed{concentration}$ of a product/reactant $ \boxed{over time}$ $\Rightarrow$ typical units a$

Sign up to see the contentIt's free!

Access to all documents

Improve your grades

Join milions of students

By signing up you accept Terms of Service and Privacy Policy

Page 1: Rate Equations and Experimental Analysis

This page focuses on rate equations and experimental methods for determining reaction orders.

Definition: A rate equation expresses the rate of a reaction in terms of the concentrations of reactants and a rate constant.

The page outlines a model answer structure for analyzing experiments to determine reaction orders:

Compare experiments where only one reactant concentration changes.
Observe how the rate changes with concentration changes.
Determine the order of each reactant based on these observations.

Example: If doubling [A] increases the rate by a factor of 4, the order with respect to A is 2.

The page also covers concentration-time graphs for different reaction orders:

Highlight: The shape of concentration-time graphs depends on the overall order of the reaction:

First order: exponential decay

Second order: reciprocal plot

Third order: more complex curve

Determining Rate Constants

The method for calculating rate constants is explained:

Rearrange the rate equation to solve for k.
Substitute values from one of the given experiments.

Example: For a rate equation Rate = k[A]²[B], rearrange to k = Rate / ([A]²[B]) and substitute values.

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Stefan S

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Samantha Klich

Android user

Anna

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Best app on earth! no words because it’s too good

Thomas R

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Basil

Android user

David K

iOS user

Sudenaz Ocak

Android user

In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.

Greenlight Bonnie

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Android user

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Elisha

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Paul T

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Stefan S

iOS user

Samantha Klich

Android user

Anna

iOS user

Best app on earth! no words because it’s too good

Thomas R

iOS user

Basil

Android user

David K

iOS user

Sudenaz Ocak

Android user

In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.

Greenlight Bonnie

Android user

Rohan U

Android user

Xander S

iOS user

Elisha

iOS user

Paul T

iOS user