Check out our library of 3D study guides and simulations to understand important concepts in chemical kinetics like collision theory, activation energy, reaction order, catalysts, and more!

Chemistry

Chemistry is the branch of science that deals with the study of matter! Did you know that chemistry is also called “the central science,” because of its role in bridging physics with other natural sciences? Let's dive into learning more on the composition and the physical and chemical properties of various forms of matter!  

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AP Bio

CBSE Bio

General Chemistry

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General Physics 

Biology

Physics

## INTRODUCTION

We have all seen a speedometer. These devices are used to measure the speed of any moving object. We generally see them in our cars or bikes, and they play a very important role by giving us an idea of how fast we are moving and whether we need to slow down (if we are going over the speed limit) or increase our speed if we are in a hurry. 

A chemical reaction that’s taking place also has a speed. This tells us how soon a reaction will be completed (all the reactants converted into products). The speed of a chemical reaction is measured by the rate law, which we are going to discuss in detail:

![Speedometer](//images.ctfassets.net/4yflszkpcwkt/4e3iB0bgtx3reLlmwny1Sk/ea621cbcaa5d98d3429a21430f8855ee/Speedometer.png)
[Source](https://auto.howstuffworks.com/car-driving-safety/safety-regulatory-devices/speedometer.htm)

### RATE LAW

The mathematical link between the speed of a reaction and the concentrations of the reagents is known as the rate law for a chemical process. 
For a general equation, 

aA+bB → C 

With no intermediary stages in its reaction process, the rate is provided by: 

r=k[A]x[B]y

![Rate law](//images.ctfassets.net/4yflszkpcwkt/23pWMia0rPcHJsV38qNbyd/e223d7616fba92f10c0f9d4d89dd73c5/rate-20law.jpeg)
[Source](https://courses.lumenlearning.com/boundless-chemistry/chapter/the-rate-law-concentration-and-time/)

### ZERO-ORDER REACTIONS

Unlike some of the other orders of reaction, a zero-order reaction has a rate that is independent of the reactant concentration. As a result, raising or reducing the concentration of the reactive species does not affect the rate of the reaction. Zero-order reactions occur when a component that is necessary for the reaction to progress, such as a substrate or a catalyst, is saturated by the reactants.

### FIRST-ORDER REACTIONS

Only one reactant's concentration determines the outcome of a first-order reaction. As a result, a first-order reaction is often known as a unimolecular reaction.

## CONCLUSION 
- The mathematical link between the speed of a reaction and the concentrations of the reagents is known as the rate law for a chemical process.
- A series of experiments with varied initial amounts of reactants must be undertaken to experimentally ascertain a rate law.

### FAQs: 

__1. How do you determine the rate law?__

A rate law depicts how the rate of a chemical reaction is affected by the concentration of reactants. The rate rule for a reaction like aA → product is usually in the form rate = k[A]ⁿ, where k is a proportionality factor termed the rate constant, and n is the reaction order with respect to A.

__2. Why is determining a rate law important?__

The pace of a chemical reaction is possibly its most crucial attribute since it determines whether a reaction can occur. Using the rate law, which is an equation that connects the rate to the concentrations of reactants, can aid a chemist in fine-tuning the reaction conditions for a better rate.

__3.  What factors affect rate law?__
Many factors impact the pace of a chemical reaction, including reactant concentration, surface area, temperature, and catalysts.

*We hope you enjoyed studying this lesson and learned something cool about __Determining the Rate Law from Experimental Data__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun, VR classrooms - we promise, it makes studying much more fun!* 😎 

## SOURCES:
1. Determining the Rate Law from Experimental Data. https://www.ck12.org/c/chemistry/determining-the-rate-law-from-experimental-data/lesson/Determining-the-Rate-Law-from-Experimental-Data-CHEM/. Accessed 7 Feb 2022.
2. The Rate Law: Concentration and Time. https://courses.lumenlearning.com/boundless-chemistry/chapter/the-rate-law-concentration-and-time/. Accessed 7 Feb 2022.


The mathematical link between the speed of a reaction and the concentrations of the reagents is known as the rate law for a chemical process.


 Determining the Rate Law from Experimental Data Study Guide

## INTRODUCTION

The curdling of milk is a natural phenomenon. It is very common in our households when the milk is left out in the open for a long time. Curdled milk is used to make cheese. But the industrial level manufacturing of cheese cannot rely on waiting for the milk to curdle. So, what do you think they do? 🤔
They induce curdling in the milk by adding a catalyst or a reagent that enhances the speed of the process. Similar is the case with chemical reactions! When we need to increase the reaction speed, we simply add a catalyst to the reaction.

![Curdling of milk](//images.ctfassets.net/4yflszkpcwkt/5NRZOAwT42zFNP9GEpnD5L/1554ec18e801cde6c632f63b6c8b649b/Curdling_of_milk.png)
[Source](https://www.cookingrevived.com/handy-cooking/cooking-hacks/what-to-do-if-milk-curdles-when-boiling/)

### CATALYSTS

- In chemistry, a catalyst is any material that speeds up a process without being utilized.
- In general, catalytic activity is a chemical interaction between a catalyst and a reactant that produces chemical intermediates that can react more rapidly with each other or with another reactant to produce the desired end product.
- The catalyst is replenished during the reaction between the chemical intermediates and the reactants.
- Several chemical manufacturing processes rely on catalyzed reactions.

![catalyst-activation-energy-reduction](//images.ctfassets.net/4yflszkpcwkt/3SXfCuofZqNvfV2sdvfFHT/e695a101c82a2dea363ee47ab0f47fb3/catalyst-activation-energy-reduction.jpg)
[Source](https://www.fuelcellstore.com/fuel-cell-components/catalyst)

### INTERMEDIATES

- A reaction intermediate, also known as an intermediate, is a molecular unit generated from reactants that interacts further to produce the immediately seen products of a chemical reaction. 
- Most chemical reactions are sequential, meaning they require more than one basic step to finish. Except for the penultimate stage, which produces the final product, each phase produces an intermediate. 
- Reactive intermediates are hardly ever segregated and generally have a brief life span. They also do not stay in the product combination due to their limited lifespan.

![reactive intermediate](//images.ctfassets.net/4yflszkpcwkt/2nxQpOqtrmgrreyAzHbxap/97d3dba65451e20a9dfb22a4db368f2b/reactive_intermediate01.png)
[Source](http://www.chem.ucla.edu/~harding/IGOC/R/reactive_intermediate.html)

## CONCLUSION

- Catalyst is any material that speeds up a process without being utilized.
- A reaction intermediate is a molecular unit generated from reactants that interacts further to produce the immediately seen products of a chemical reaction.
- The catalyst is replenished during the reaction between the chemical intermediates and the reactants.

### FAQs: 

__1. What is a catalyst in chemistry?__

A catalyst is any material that speeds up a process without being depleted.

__2. Do catalysts affect intermediates?__

Catalysts often react with one or more reactants to produce intermediates, providing the ultimate reaction product renewing the catalyst in the procedure. So yes, catalysts determine which intermediate will be formed in a reaction.

__3.  What are the differences between an intermediate and a transition state?__

The difference between an intermediate and a transition state is that an intermediate has a discontinuous duration (ranging from a few nanoseconds to several days). However, a transition state only lasts for one bond vibration cycle. An intermediate might be a very unstable compound (an unstable intermediate) or a stable compound (a non-reactive intermediate).

__4. Is a catalyst the same as an intermediate?__

At the start of the process, a catalyst is employed, and it is then regenerated at completion. During the process, an intermediate is formed, but it vanishes at completion. Thus a catalyst is not the same as an intermediate.

*We hope you enjoyed studying this lesson and learned something cool about __Chemical Kinetics: What's the Difference Between a Catalyst and an Intermediate__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun, VR classrooms - we promise, it makes studying much more fun!* 😎 

## SOURCES:
1. Chemical Kinetics: What's the Difference Between a Catalyst and an Intermediate?. https://www.ck12.org/c/chemistry/reaction-intermediate/lecture/Chemical-Kinetics:-Whats-the-Difference-Between-a-Catalyst-and-an-Intermediate/. Accessed 7 Feb 2022.  
2. Catalyst. https://www.britannica.com/science/catalyst. Accessed 7 Feb 2022


A catalyst is any material that speeds up a process without being utilized.


Chemical Kinetics: What's the Difference Between a Catalyst and an Intermediate? Study Guide

## INTRODUCTION

Reactions such as rusting take a lot of time to occur, while a neutralization reaction, i.e., when an acid reacts with a base, takes almost no time. So how fast or slow a reaction is, is called the rate of reaction, and the rate of reaction depends on the order. You must be wondering what reaction order is in chemistry? Let’s understand.

### REACTION ORDER

Order of reaction is the sum of the power of concentration of reactants written in rate law expression. Let’s understand in simple words.
The rate of a reaction depends or sometimes doesn’t depend on the concentration of reactants. 

Reaction rate = is the change in the amount of a reactant or product per unit time.

So, the reaction order is the relationship between the concentrations of species and the rate of a reaction. The order of reaction can be any integer or fraction. It can be found out only experimentally. 

### DIFFERENT RATE ORDERS

### ZERO-ORDER REACTIONS:

                                     A → B

Here, the rate is independent of the concentration of the reactant, which is expressed as [A]. 

                                 Rate =  k[A]0

The power of [A] is 0, and hence the order of the reaction is zero. This means the rate of reaction won’t change even if we increase or decrease the concentration of the reactant.

![DIFFERENT RATE ORDERS](//images.ctfassets.net/4yflszkpcwkt/1PdK2kkJWjSDUMnJJlhRM1/f9a6b367d97daa557db1083343a092aa/14.16.jpg)
[Source](https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/05%3A_Experimental_Methods/5.07%3A_Using_Graphs_to_Determine_Integrated_Rate_Laws)

### FIRST-ORDER REACTIONS:

                                    A → B

Here, the rate of reaction is proportional to the concentration of A. This means as [A] increases, the rate of reaction increases too and vice versa.

                                Rate = k [A]

Since the power of [A] is 1, the order of the reaction is 1. The rate depends linearly on the concentration of reactant here. 
The rate of reaction is the slope of the graph.  

### SECOND-ORDER REACTION:

                                  A + B → C

Here, the rate is expressed as k [A] [B], which means the rate will be dependent on both of the reactants A and B. If we increase or decrease the concentration of any of these, then the rate will change. 

The rate is proportional to [A], and the order for A is 1, and the same is for B. But the overall order is the sum of orders with respect to both the reactants, so it will be 2.

## CONCLUSION:
- Order of reaction is the sum of the power of concentration of reactants written in rate law expression.
- It can be an integer or fraction. 

### FAQs:

__1. What is the order of a reaction?__

Order of reaction is the sum of the power of concentration of reactants written in rate law expression.

__2. Can the order of reaction be -½?__

Yes, the order of the reaction can be an integer or fraction.

__3. For Rate = k [A], what is the order of reaction?__

Since the power of concentration of reactant is 1, the reaction is of the first order.

*We hope you enjoyed studying this lesson and learned something cool about __Reaction Order__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎

## SOURCES:
1. Reaction Order: https://www.ck12.org/c/chemistry/reaction-order/lesson/Order-of-Reaction-CHEM/?referrer=concept_details. Accessed 8th March 2022.
2. Reaction Order: https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/03%3A_Rate_Laws/3.03%3A_The_Rate_Law/3.3.03%3A_Reaction_Order. Accessed 8th March 2022.


Order of reaction is the sum of the power of concentration of reactants written in rate law expression, and it can be an integer or fraction. 


Reaction Order Study Guide

## INTRODUCTION

Collision theory in chemistry allows scientists to predict a rate constant of a chemical reaction which can be used to determine reaction rates. This theory was developed by Max Trautz and William Lewis to derive meaningful insights into these chemical reactions.  

### WHAT IS COLLISION THEORY

Collision theory states that the rate of a chemical reaction is directly proportional to the number of collisions occurring between the reactant molecules. In simple terms, the collision theory in chemistry explains what initiates chemical reactions. Theoretically, the more that the reactant molecules collide with one another, the faster the rate of reaction becomes. In reality, however, only a small fraction of the collisions are what we term effective collisions, which are the only type of collision that results in the creation of a product.

To initiate effective collisions, reactant molecules are required to have activation energy, which is the minimum amount of energy required to undergo a reaction. The count of molecules possessing sufficient energy is all dependent on the reactant's temperature. If these reactants do not possess their required activation energy, they bounce back from each other without even reacting. 

### POSTULATES OF COLLISION THEORY

Collision theory is based on three postulates:
The rate of reaction is proportional to the rate of reactant collision molecules. 
The reacting element should collide to allow contact between the atoms, which are meant to be bonded together. 
There must be sufficient energy to allow mutual penetration of the reactants so that the electrons can again arrange and form new bonds. 

## CONCLUSION

- Collision theory occurs at certain chemical reactions and rates. 
- The fundamental principle is that in order to react, molecules must undergo effective collisions. 
- In order to undergo an effective collision, the molecules’ collision energy must be greater than or equal to activation energy during the reaction.
- Reactants with low concentration result in few collisions, and those with high concentrations produce more collisions. 

### FAQs

__1. What is collision theory?__

Collision theory defines that the chemical reaction rate is proportional to the number of collisions occurring between the reactant molecules. This occurs at certain chemical reactions and rates. 

__2. What are the 4 points of collision theory?__

- Reactants must collide in the proper orientation.
- Collision energy must be greater than or equal to activation energy during the reaction. 
- The reactant particles must collide with one another.
- The collision frequency should be larger than the number of factors for the reaction. 

__3. What are the three postulates of collision theory?__

- The rate of reaction is proportional to the rate of reactant collision molecules. 
- The reacting molecules must collide to allow contact between the atoms, which are meant to bond together. 
- There should be sufficient energy to allow joint penetration of the reactants so that the electrons can rearrange and form new bonds.

__4. What equation is used for collision theory?__

K ∝ e-Ea/RT

K = A e-Ea/RT

where, A is the frequency factor, Ea is the activation energy, R is gas constant and T is the absolute temperature

This is the Arrhenius equation, and the collision theory equation is accommodated in this only. 

![molecular-collisions](//images.ctfassets.net/4yflszkpcwkt/5p5vzbgw5cwJchDyzvs47n/bfa4617684bd7d1ab35ee5ab311037bd/molecular-collisions.jpeg)
[Source](https://courses.lumenlearning.com/introchem/chapter/the-collision-theory/) 

*We hope you enjoyed studying this lesson and learned something cool about __Collision Theory__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our app to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎

## SOURCES: 

1. The Collision Theory: https://courses.lumenlearning.com/introchem/chapter/the-collision-theory/. Accessed 28 Feb 2022.
2. The Collision Theory: https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Kinetics/06%3A_Modeling_Reaction_Kinetics/6.01%3A_Collision_Theory/6.1.06%3A_The_Collision_Theory. Accessed 28 Feb 2022.
3. Kinetics and Collision Theory: http://dept.harpercollege.edu/chemistry/chm/100/dgodambe/thedisk/kinetic/6back.htm. Accessed 28 Feb 2022.


Collision Theory plays a vital role in this fast-developing world and results in chemical reactions.

Collision Theory Study Guide

## INTRODUCTION
Have you ever looked at trees and wondered if the branches at the canopy would fall faster than the branches near the ground? That is because the former has more potential energy than the latter. 

![tree-branches potential energy](//images.ctfassets.net/4yflszkpcwkt/1BgeFA3EDimt6Hsg93HiIo/d88b38cdd194f6a1df1eed92cb807ccd/tree-branches.jpg)
[Source](https://byjus.com/physics/potential-energy/#potential%20energy%20formula)

### POTENTIAL ENERGY DIAGRAMS
The change in potential energy in a chemical reaction could be plotted on a potential energy diagram, and we can depict these changes in a potential energy graph. 

### ENDOTHERMIC REACTION & EXOTHERMIC REACTION
In the figure below, you can see energy diagrams of 
(A) Endothermic reaction
(B) Exothermic reaction

Here, (ΔH) denotes the change in enthalpy.

Enthalpy, normally denoted H, is a thermodynamic property; it is equal to the sum of the internal energy plus the product of the pressure and the volume.

Endothermic reactions have a positive (ΔH), whereas exothermic reactions have a negative (ΔH), as shown in this figure:

![Potential Energy Diagrams](//images.ctfassets.net/4yflszkpcwkt/WVNhWV0SqLqzUGztlYivW/4f4dfb83cdc8e44df3c64c0c6bfbcad0/CK12_Screenshot_18-4-1.png)
[Source](https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/18%3A_Kinetics/18.04%3A_Potential_Energy_Diagrams#:~:text=A%20potential%20energy%20diagram%20shows,reactants%20are%20converted%20into%20products.&text=The%20activation%20energy%20for%20a,the%20reactants%20and%20the%20products.)

Here, the whole potential energy declines as it releases the energy to the surrounding environment.

### READING ENERGY DIAGRAMS - ENDOTHERMIC GRAPH AND EXOTHERMIC GRAPH

In the above figure, you can interpret the energy diagrams as:

(A) In the endothermic reaction graph, the energy of resultant products is more than reactants (ΔH is a positive enthalpy change). Here, the total potential energy rises as energy is absorbed from the surrounding environment.

(B) In the exothermic reaction graph, the energy of the resulting products is less than reactants (ΔH is a negative enthalpy change). Here, the total potential energy declines as it releases energy.

### ACTIVATION ENERGY DIAGRAM
The highest point of the curve between reactants and products in the potential energy diagram shows you the activation energy for a reaction. When particles react, they must have enough energy to collide to overpower the barrier.

__Activation Energy Diagram:__

![Potential Energy Diagrams](//images.ctfassets.net/4yflszkpcwkt/645xqAkQQw1pMDPfxaYXI2/bcc038a5fe10d000a220ad6e48ab03af/CK12_Screenshot_18-4-2.png)
[Source](https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/18%3A_Kinetics/18.04%3A_Potential_Energy_Diagrams#:~:text=A%20potential%20energy%20diagram%20shows,reactants%20are%20converted%20into%20products.&text=The%20activation%20energy%20for%20a,the%20reactants%20and%20the%20products.)

Here, the activation energy is denoted by (Ea).

(A)  Ea is lower, as there is a downward dip implying the reaction is quick.

(B) Ea is higher, implying the reaction is quite slow.

### Continue your learning journey
Learn about [Potential Energy ](https://assets.ctfassets.net/4yflszkpcwkt/50QYKzoj4AU90tBzjtJqSa/3a43f72a850aad753f7416e5eb860664/TL_DR_Potential_Energy_Diagrams.pdf)

Learn about [Kinetic Energy ](https://www.inspiritvr.com/chemistry/measurements/kinetic-energy-study-guide)

## CONCLUSION:
- You can depict changes in the potential energy of a system in a potential energy diagram.
- Graphs of both endothermic and exothermic reactions and how to read them have been discussed.
- Explanation of diagram of activation energy on how the process works.

### FAQs:

__1. How do you read an energy diagram?__

Potential energy diagrams can be read from the X-axis to the reaction line. Dashed lines on the graph visualize the potential energy in the graph.

__2. What does an energy diagram tell you?__

An energy diagram shows whether a reaction is endothermic or exothermic, the potential energy of the reactants and products, and the change in energy for such a reaction.

__3. Is delta H negative for exothermic?__

Yes, delta H is negative in the graph of an exothermic reaction.

*We hope you enjoyed studying this lesson and learned something cool about __Potential Energy Diagrams__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our app to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎 

## SOURCES:
1. Potential Energy Diagrams. https://www.ck12.org/c/chemistry/potential-energy-diagrams/lesson/Potential-Energy-Diagrams-CHEM/. Accessed 17 Feb 2022. 
2. Potential Energy Diagrams. https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/18%3A_Kinetics/18.04%3A_Potential_Energy_Diagrams#:~:text=A%20potential%20energy%20diagram%20shows,reactants%20are%20converted%20into%20products.&text=The%20activation%20energy%20for%20a,the%20reactants%20and%20the%20products. Accessed 17 Feb 2022. 


A diagram showing the total potential energy of a reacting system as the reaction proceeds are known as a potential energy diagram.


Potential Energy Diagrams Study Guide

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## INTRODUCTION

What is the reaction rate? It is the measure of how fast a chemical reaction proceeds. Consider a combustion reaction like the burning of wood, which takes place in a few hours as compared to rusting which can take several days.

![Fire-combustion-fuel](//images.ctfassets.net/4yflszkpcwkt/2UUhCAzgbj32ViMj1fxFoT/24d1dcaf386159afa81aa2e006e61d07/Fire-combustion-fuel.jpg)
[Source](https://www.britannica.com/science/combustion)

- In a chemical reaction, where A & B  are the  reactants and AB is the product or A B → AB.
- The reaction rate in chemistry is determined by how fast the concentration of A & B increases or decreases. 

![Rate-of-a-Reaction](//images.ctfassets.net/4yflszkpcwkt/5y9e3HuUBddpWe0LyBxSV7/81f3a9a2914da71ac1307bad2543f08a/Rate-of-a-Reaction.jpg)
[Source](https://qsstudy.com/definition-rate-reaction/)

### DEFINITION OF THE RATE OF REACTION
It is defined as the estimate of the conversion in the concentration of the reactants through a certain time interval. It may be expressed as 

               Rate = Δ concentration / Δ time

According to the above reactants A & B, the reaction rate may be written as:

                Rate = - Δ (A) / Δ t

                Rate = - Δ (B) / Δ t

                Rate =   Δ (AB) / Δ t

Here Δ(A) is the difference in the concentration of reactant A through time (t₂ - t₁). The bracket indicates the concentration in Molarity of the substance, and the negative signs show the decrease in the concentration of only the reactants.

Therefore, Δ(A) = (A₂) – (A₁) where A₂ is the final concentration and A1 is the initial concentration of reactant A. It will always be negative since the concentration of the reactant decreases with time during the reaction.

### HOW TO FIND THE RATE OF A REACTION?

A reaction rate is the conversion of the concentration of reactants with time. A 2.00M solution of A reacts with B to form AB from the above equation. It takes place in 20 seconds, and the concentration of A drops from 2.00M to 0.72M. 
Rate can be calculated as Δ(A) = (A₂) – (A₁) / Δ t    

Therefore, 

          Rate = 0.72M – 2.00 M / 20 s  

                = -(-1.28) M / 20 s  

                = 0.064 M/s

The reaction rate unit is measured in molarity per second or M/s. So for the above example, A's molarity decreases at a rate of  0.064 seconds. 

## CONCLUSION: 

- The reaction rate in chemistry is the difference in the concentration of a reactant or product divided by the time taken.
- The rate of a reaction is measured as molarity per second. 

## FAQs:

__1. How do you calculate the rate of a reaction per second?__

It is calculated as rate or Δ (A) = (A₂) – (A₁) / Δ t   

__2. How do you calculate the rate of reaction from molarity?__

If the initial Molarity of a reactant was 1.00M and the final Molarity changes to 0.64M over 15 seconds, then the rate of the  reaction is calculated as 

Rate = 0.64M – 1.00 M / 15 s  

= -(- 0.36) M / 15 s  

= 0.024 M/s

The rate of the reaction is expressed as 0.024M/s.

__3. What is the rate of reaction formula?__

The rate may be calculated as:          

rate = - Δ (A) / Δ t

*We hope you enjoyed studying this lesson and learned something cool about the __Chemical Reaction Rate__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎

## SOURCES:

1. Reaction Rate. https://www.ck12.org/c/chemistry/reaction-rate/lesson/Chemical-Reaction-Rate-CHEM. Accessed 17 February 2022.
2. Reaction Rate. https://www.britannica.com/science/reaction-rate. Accessed 18 February 2022.

The reaction rate in chemistry is the speed of a chemical reaction.


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