AP Chemistry Unit 7 Review: Equilibrium!

Cararra
27 Apr 202011:19
EducationalLearning
32 Likes 10 Comments

TLDRThe video script discusses the concept of chemical equilibrium, emphasizing the equilibrium constant as a critical factor in understanding how reactions balance themselves. It explains the relationship between reactants and products, and how to calculate the equilibrium constant based on their concentrations or pressures. The script also delves into how changes in conditions such as temperature, reactant amounts, and container size can shift equilibrium. Furthermore, it clarifies the difference between KP and KC, and concludes with an explanation of rate laws, focusing on the rate-determining step and how to derive the overall rate law for a reaction.

Takeaways
  • 🌟 Chemical equilibrium refers to the state where reactions balance themselves without indicating the speed of balancing.
  • πŸ“ˆ The equilibrium constant (K) is crucial for understanding chemical equilibrium; it's the ratio of products to reactants.
  • πŸ”„ At equilibrium, forward and backward reactions occur simultaneously, with their rates being equal.
  • πŸŽ“ When calculating the equilibrium constant, ignore solids and liquids, focusing only on gases and solutions.
  • πŸ”’ The equilibrium constant expression is built using the concentrations of products raised to their stoichiometric coefficients and placed over reactants' concentrations.
  • πŸ”„ For Kc (concentration constant), use concentrations, and for Kp (pressure constant), use pressures instead.
  • πŸ’‘ The equilibrium constant K value indicates how favored the products are over the reactants; a large K means more product concentration is favored.
  • πŸ“Š The reaction quotient (Q) is used to determine the direction a reaction will proceed in; compare Q to K to know if the reaction will favor products or reactants.
  • βš–οΈ Le Chatelier's principle states that a system will adjust to counteract changes made to it, such as adding reactants or increasing temperature.
  • πŸš€ Rate laws are determined by identifying the rate-determining step (the slowest step) and using it to express the overall rate of the reaction.
Q & A
  • What is the main topic of the video?

    -The main topic of the video is chemical equilibrium, specifically focusing on how chemical reactions balance themselves.

  • What does the term 'equilibrium' mean in the context of chemistry?

    -In chemistry, 'equilibrium' refers to a state where the forward and backward reactions occur at the same rate, resulting in a balance without any net change in the concentrations of reactants and products.

  • What is the equilibrium constant and why is it important?

    -The equilibrium constant, denoted as K, is the ratio of the concentration of products to the concentration of reactants raised to the power of their respective stoichiometric coefficients. It is important because it provides a measure of the extent to which a reaction favors the formation of products over reactants at a given temperature.

  • How does one calculate the equilibrium constant for a given reaction?

    -To calculate the equilibrium constant, K, one must express it as the product of the concentrations of the products raised to the power of their stoichiometric coefficients in the balanced chemical equation, divided by the product of the concentrations of the reactants raised to the same powers.

  • What is the significance of the equilibrium constant value in predicting the direction of a reaction?

    -A large K value indicates that the reaction favors the formation of products, while a small K value suggests that the reaction favors the formation of reactants. If the reaction quotient (Q) is greater than K, the reaction will shift towards the reactants, and if Q is less than K, the reaction will shift towards the products.

  • What are the different types of equilibrium constants and how do they differ?

    -Different types of equilibrium constants include K, Kp, Ka, Kb, and Kw. They differ based on the units used for their expressions, with K typically using concentration units (M), Kp using pressure units (atm), and Ka, Kb, and Kw being specific to acid dissociation, base dissociation, and water dissociation, respectively.

  • How does changing the concentration of a reactant affect the position of equilibrium?

    -Increasing the concentration of a reactant will shift the equilibrium towards the products to counteract the change, according to Le Chatelier's principle. This is because the system tries to reduce the concentration of the added reactant by forming more products.

  • What happens when the temperature is increased for an exothermic reaction?

    -For an exothermic reaction, increasing the temperature will cause the equilibrium to shift in the direction that absorbs heat, which is towards the reactants. This is because the system tries to reduce the added heat by favoring the endothermic process (formation of reactants).

  • How does the size of the container affect the equilibrium of a reaction involving gases?

    -Changing the size of the container affects the equilibrium of reactions involving gases by altering the number of gas molecules on each side of the reaction. If the container size is reduced, the reaction will shift towards the side with fewer gas molecules to reduce the pressure increase caused by the smaller volume.

  • What is the rate-determining step in a chemical reaction?

    -The rate-determining step is the slowest step in a chemical reaction mechanism. It determines the overall rate of the reaction because the faster steps will adjust to match the rate of the slowest step, causing a 'traffic jam' at this step.

  • How can one determine the overall rate law of a reaction?

    -To determine the overall rate law, one must first identify the rate-determining step. Then, using the stoichiometric coefficients from this step, an expression for the rate law can be written. This expression is then modified using equilibrium expressions to eliminate any intermediates that are not present in the reactants or products.

Outlines
00:00
πŸ“š Introduction to Chemical Equilibrium

The paragraph introduces the concept of chemical equilibrium, explaining it as a balance between reactants and products in a chemical reaction without indicating the speed of the reaction. It emphasizes the importance of the equilibrium constant (K), which is the ratio of the concentration of products to the concentration of reactants. The explanation includes an example of the Haber-Bosch process for synthesizing ammonia and clarifies that the equilibrium constant is independent of the reaction speed. The paragraph also discusses how to calculate the equilibrium constant and the significance of the equilibrium constant in determining the favorability of products over reactants.

05:01
πŸ”„ Understanding the Equilibrium Constant (K)

This paragraph delves deeper into the equilibrium constant (K), explaining how it can be used to predict the direction in which a reaction will proceed. It introduces the concept of the reaction quotient (Q), which is used to compare the current state of a reaction to the equilibrium state. The discussion includes how changes in concentration, temperature, and pressure can shift the equilibrium position. The paragraph also briefly touches on the differences between KP (related to pressure) and KC (related to concentration), and the implications of these differences. Lastly, it provides a brief overview of how changes in the system, such as increasing a reactant or decreasing container size, can affect the direction of the reaction.

10:02
πŸ§ͺ Determining Rate Laws and Reaction Mechanisms

The final paragraph focuses on the process of determining rate laws for chemical reactions. It explains that the rate of the overall reaction is determined by the slowest step, known as the rate-determining step. The paragraph outlines the method for identifying this step and using it to derive the overall rate law. It also discusses how equilibrium expressions can be used to eliminate intermediates from the rate law equation. The explanation includes an example of how to derive a rate law by considering the slow step and the equilibrium expression, ultimately showing how to arrive at a simplified rate law expression.

Mindmap
Changing Container Size
Increasing Temperature
Adding Reactants
Substitution and Elimination
Equilibrium Considerations
Identifying the Slow Step
Shift in Equilibrium
Q Value
Types of Equilibrium Constants
Ignoring Solids and Liquids
Equilibrium Expression
Forward and Backward Reactions
Equilibrium Constant (K)
Balance in Reactions
Examples
Response to Changes
Deriving Rate Laws
Elementary Reactions
Rate-Determining Step
Direction of Reaction
Calculating the Equilibrium Constant
Definition and Concept
Le Chatelier's Principle
Reaction Rate Laws
Chemical Equilibrium
Chemical Equilibrium and Reaction Dynamics
Alert
Keywords
πŸ’‘Chemical Equilibrium
Chemical Equilibrium refers to the state in a chemical reaction where the concentrations of reactants and products remain constant over time. It is a dynamic balance where the forward and reverse reactions occur at the same rate. In the video, the concept is central to understanding how chemical reactions balance themselves, and the speaker emphasizes that equilibrium does not provide information on the speed of the reaction but rather the point at which the reaction achieves balance.
πŸ’‘Equilibrium Constant (K)
The equilibrium constant (K) is a measure of the extent to which a reaction proceeds. It is the ratio of the concentration of products to the concentration of reactants, each raised to the power of their stoichiometric coefficients in the balanced chemical equation. A large K value indicates that the reaction favors the formation of products, while a small K value suggests that the reaction favors the reactants. In the video, the speaker explains that understanding K is crucial for grasping chemical equilibrium and that it can be used to predict the direction in which a reaction will proceed.
πŸ’‘Rate Laws
Rate laws describe the relationship between the rate of a chemical reaction and the concentrations of the reactants. They are used to predict how changes in concentration will affect the rate of a reaction. The video emphasizes the importance of identifying the rate-determining step, which is the slowest step in a reaction sequence that dictates the overall rate of the reaction. The speaker explains how to derive rate laws by considering the stoichiometry of the reaction and the equilibrium constant.
πŸ’‘Le Chatelier's Principle
Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, such as concentration, pressure, or temperature, the position of equilibrium moves to counteract the change. This principle helps predict how a system at equilibrium will respond to external changes. In the video, the speaker explains how increasing reactants or temperature, or decreasing container size, can shift the equilibrium position, either towards the production of more products or reactants.
πŸ’‘Stoichiometric Coefficients
Stoichiometric coefficients are the numbers that appear in front of the chemical formulas in a balanced chemical equation, indicating the number of moles of each reactant or product involved in the reaction. These coefficients are crucial for calculating the equilibrium constant and rate laws. In the video, the speaker uses these coefficients to determine the powers in the equilibrium expression and to balance the rate law equation.
πŸ’‘Reactants and Products
Reactants are the substances that are consumed in a chemical reaction, while products are the substances that are formed as a result of the reaction. Understanding the relationship between reactants and products is fundamental to studying chemistry, as it helps to predict and explain the outcomes of reactions. In the video, the speaker discusses how the balance between reactants and products is crucial for chemical equilibrium and how the equilibrium constant reflects this balance.
πŸ’‘Dynamic Balance
A dynamic balance refers to a state in a chemical reaction where the forward and reverse reactions occur at equal rates, resulting in constant concentrations of reactants and products. This concept is essential for understanding chemical equilibrium, as it highlights that equilibrium is not a static state but an ongoing process. In the video, the speaker explains that chemical equilibrium is a dynamic balance, with the forward and reverse reactions happening simultaneously.
πŸ’‘Concentration
Concentration refers to the amount of a particular substance present in a given volume or mass. In the context of chemistry, it is a critical factor that influences the rate of reactions and the position of chemical equilibrium. The video discusses how concentration affects the equilibrium constant and how changes in concentration can shift the equilibrium position.
πŸ’‘Pressure
Pressure is the physical quantity that is exerted by gases or liquids on the walls of their container. In the context of chemical reactions involving gases, pressure can influence the position of chemical equilibrium. According to the video, changes in pressure can affect the rate at which gases react and the equilibrium constant, especially when the number of gas molecules on each side of the reaction equation is different.
πŸ’‘Temperature
Temperature is a measure of the average kinetic energy of the particles in a substance. It plays a significant role in chemical reactions, affecting both the rate of reactions and the position of chemical equilibrium. The video explains that increasing the temperature can shift the equilibrium in the direction that absorbs heat, especially for exothermic reactions.
πŸ’‘Gas Molecules
Gas molecules are the individual atoms or groups of atoms that exist in the gaseous state. In chemical reactions, the number and type of gas molecules can influence the position of chemical equilibrium, particularly when considering the effects of pressure and volume. The video discusses how the number of gas molecules on each side of a reaction can determine the direction in which the equilibrium will shift when the container size is changed.
Highlights

Introduction to chemical equilibrium and its significance in balancing chemical reactions.

Explanation of the equilibrium constant, its role as the ratio of products to reactants, and its importance in understanding chemical balance.

Discussion on how the equilibrium constant cannot provide information about the speed of reactions, but only the point of balance.

Clarification on the difference between various types of equilibrium constants such as K, Kb, Kp, and Kw, and their relevance to specific scenarios.

Explanation of how to calculate the equilibrium constant (K) for a given reaction, using the example of the Haber-Bosch process.

Importance of considering the physical state of reactants and products when calculating equilibrium constants, with the exclusion of solids and liquids.

Illustration of how the equilibrium constant (K) value indicates the favorability of products over reactants, and its implications for reaction direction.

Use of the reaction quotient (Q) to determine the direction a reaction will proceed from a non-equilibrium state, and comparison of Q with K.

Explanation of how changes in system conditions like concentration, temperature, and pressure can affect the direction of a chemical reaction.

Discussion on the difference between KP (involving pressure) and KC (involving concentration), and the relationship between them.

Overview of Le Chatelier's principle and its application to predict how a system will respond to changes in reactants, temperature, and container size.

Introduction to rate laws and the concept of the rate-determining step in chemical reactions.

Methodology for determining the overall rate law of a reaction by focusing on the slow step and utilizing equilibrium expressions.

Explanation of how to manipulate and simplify rate laws using equilibrium expressions to eliminate intermediate species.

Final thoughts on the importance of understanding rate laws for predicting reaction outcomes and the practical applications of this knowledge.

Transcripts
00:00

all right if your boy kirara with

00:01

another camp crash course all right I

00:04

draw anything out of context probably

00:05

think I really cringe but I'm actually

00:06

not okay

00:07

oh hi I'm moving on moving on okay hello

00:11

everybody I'm Cara and today we are

00:13

going to be talking about chemical

00:15

equilibrium if you weren't able to read

00:17

that but you probably couldn't how I

00:18

wrote it but we're going to be talking

00:20

about how chemical reactions

00:22

balance themselves so that's what

00:23

equilibria mean now because it means

00:25

balance it doesn't tell you anything

00:27

about the speed at which it balances it

00:28

just says where it balances that's all

00:30

the chemical equilibrium can't tell you

00:32

so do not try to figure out how fast the

00:34

reaction is happening by using anything

00:36

we talked about in this video except at

00:38

the end we'll have a little compute on

00:39

that so now the most important thing to

00:41

understand about equilibrium is the

00:43

equilibrium constant because once you

00:45

understand equilibrium constant

00:46

everything else falls into place

00:47

basically the equilibrium constant is

00:50

the ratio of your product to reactor so

00:53

let us say beyond the reaction and 2 + 3

00:56

H to yield to nh3 this basically the

01:00

haber-bosch model oops I forgot my

01:01

backward error don't forget in

01:03

equilibrium your lies have forward and

01:04

backward reactions happening at the same

01:06

time and the definition of equilibrium

01:08

the one though they're equal so let's

01:09

say we wanted to find the equilibrium

01:10

constant of the reaction symbolize K now

01:13

what I'm finding the equilibrium

01:14

constant I don't care Oh like it doesn't

01:17

even cross my mind whether it's k KS p k

01:20

a.kb

01:20

KW i don't care just keep to yourself ok

01:23

I'm good we don't care the only thing I

01:25

care about in the reaction and the phase

01:27

is a matter of the reaction reactants

01:29

and products so let's write it all you

01:31

guys thankfully are gases so when you're

01:33

finding the equilibrium constant you

01:34

basically go with the product first and

01:36

you say it needs to be the first product

01:38

and we basically symbolize it with

01:39

concentration of nh3

01:41

you guys are concentration or you can do

01:43

pressure and then you take this

01:44

coefficient that's in front of it and

01:45

you put it to the power of that so we do

01:48

n HP squared and then in the denominator

01:49

we gotta do the reactants so we first

01:52

got n2 which does not have a which has a

01:55

coefficient of 1 so we don't put a power

01:56

and then we have h2 which is coated in 3

01:59

they put it a third power okay so this

02:01

is our equilibrium expression now yet be

02:04

careful because in this case we got

02:05

lucky and they're all gases but whenever

02:07

you're calculating an equilibrium

02:09

content you have to ignore solids and

02:11

liquids the only thing that matter

02:13

gases and equally a solution so you

02:15

might be asking Kirara why don't you

02:16

care whether it's K or K B or k XP or

02:19

whatever nonsense the reason in the

02:20

clause if you only care about the baby

02:22

that matter it eventually give you the

02:23

right equilibrium constant regard for

02:25

example KSP right let's see so let's say

02:27

you AG CL yields in d plus plus CL minus

02:31

and it wanted us to find the KSP of it

02:33

you might have to pay that matter we say

02:35

this solid cuz it's a solid that you

02:36

want to dissolve and then it goes into a

02:38

pH solution wants it dissolved so if we

02:41

use the same strategy meeting before we

02:42

use the products of AG plus no

02:44

covariance to deal with here co-

02:47

we don't have to put in this because of

02:49

solvent and we didn't even think about

02:51

it but we did get the KSP properly the

02:54

only thing you have to know it's a

02:55

really uh reaction and the bigger the

02:57

matter and you automatically get

02:58

everything let's do a KB and K a thing

03:00

so for K a we could say h2so4 + h2o eh -

03:05

bo + + hso4 month and basically we know

03:08

that this is aqueous this is liquid this

03:11

is aqueous and this also and then we

03:14

know that there's a k-8 because we're

03:17

dealing with an acid associating and we

03:20

don't even out worry about swaggins K

03:21

and we gonna write the equilibrium as we

03:22

always did interview a + time hso4 minus

03:26

/ h2so4 and meeting in the think about

03:29

what it means to have a k-8 we just

03:31

found the equilibrium constant for the

03:33

reaction and we are coochi game 2169 i

03:35

don't care

03:36

okay so what the heck does the k value

03:39

actually tell it tells us how much the

03:41

products are favored over the reactants

03:42

right but you're putting concentration

03:44

of products over upon the occasion of

03:45

reaction so if your K is really big that

03:49

means that you want to have a lot more

03:50

concentration of products if KT has

03:52

really small does anyone have less

03:54

products and a lot of reactants what

03:55

this should be equilibrium but anyway

03:57

another thing we can do with equilibrium

03:58

is tell us which way the reaction is

04:00

going to go from our given position so

04:02

equilibrium constant is why new system

04:05

of the equilibrium what that ratio of

04:06

equal to what your system is not always

04:09

at equilibrium right let's go back to

04:11

our Hebrew box example so let us say

04:13

that we had like 0.1 atmosphere of 83

04:16

and 0.2 atmosphere of h2 and then 0.05

04:25

atmosphere

04:26

and two I just made these numbers up so

04:28

there's no way that this is already at

04:29

equilibrium so how do we know which way

04:31

it's gonna go is it gonna make you more

04:32

three years are gonna make more NH 2

04:34

what's X at each ear and who or H 2 all

04:37

we know that by doing cute and the way

04:39

you find cute is exactly the same as

04:40

finding K except this app it's current

04:43

time what is that ratio of equal to

04:45

right now even though it might not be at

04:46

equilibrium so well calculated 0.1

04:49

squared / 0.2 times 0.05 and then this

04:53

have to be cute and basically if this Q

04:56

value is greater than our K then we know

04:58

that there's too many products because

05:00

the numerator is way bigger than the

05:02

denominator and we don't want that so

05:03

that means that the reaction is gonna

05:05

keep going left it's gonna produce more

05:07

and do an h2 because it's not yet that

05:09

you Calibri amande want to get rid of

05:10

the product it's the other way around

05:11

with it less than k then i'll go the

05:13

other way okay so that's how you use

05:14

cute cue that any instant in time cave

05:17

what it wants to be at equilibrium

05:18

all right let's quickly go over what KP

05:21

with KC is because these are the only

05:22

two that are actually different from

05:24

each other

05:24

so KP the P stands for pressure and it's

05:27

basically when you use pressures instead

05:29

of concentration because you can do that

05:31

with kids and then Casey what do you

05:32

expect

05:33

you can concentration now the way I like

05:35

to remember the difference between these

05:36

two is because like your a pressure

05:38

times volume and people to NRT by the

05:40

ideal gas on right so your n over B

05:43

which is equal to your concentration is

05:45

going to be equal to P over RT so let's

05:47

say the KP is equal to PA times PB over

05:50

PC right this corresponds to the

05:52

reaction C goes to a plus B and they

05:54

know what gas is coming out of pressure

05:56

I mean then we also know that the

05:58

canacee are going to be concentration of

05:59

a kind of concentration of B over

06:01

concentrated on steep so if we plug in

06:03

this equation for over here we get RT

06:07

squared did not fit in the numerators

06:09

denominator and then we get an RT the

06:12

first power and the denominator

06:13

denominator and we're left with the KC

06:16

is equal to PA times PB over RT PC so

06:24

basically all I'm trying to show you is

06:25

that KP and K C are very different and

06:27

if you want to see how two different

06:28

just take this equation that I showed

06:30

you and plug it in to the corresponding

06:32

concentration equation and you should be

06:34

good but anyway this like pretty

06:35

I don't think it's gonna be on the exam

06:38

I'm not sure our teacher taught us but

06:39

she mentioned it very briefly so I don't

06:41

think it would be that useful okay

06:43

okay two more things in the shack and

06:44

finding rate laws okay so the shack it

06:46

basically said that your system is gonna

06:48

contract any change in it but basically

06:49

they're like four ways in which the work

06:52

to go to haber-bosch again and here Bob

06:54

does pretty end up there make I'm pretty

06:56

sure let me just purify this wow I'm

06:58

very good at it extra EXO's exothermic I

07:01

can speak to Exeter okay so the fourth

07:04

thing that can happen is first you

07:06

increase one of the reactants so let's

07:08

NAT says it wants to undo that so how's

07:10

it gonna do that it's gonna take this

07:12

reaction towards the right because if

07:14

you increase of reactants you know I can

07:16

get rid of them you have to turn them

07:17

into more product so we'll draw an arrow

07:19

that says their equilibrium is shifting

07:21

right - in peace product exactly the

07:24

same except opposite logic okay increase

07:27

temperature the way I like to think

07:28

about this is like if going forward in

07:31

the reaction releases heat right

07:32

exotherm then if you increase the 10 you

07:36

want to get rid of heat right you don't

07:37

want to make more so instead of going

07:40

right which made more tea it'll actually

07:41

go left okay I probably computing you

07:43

more because it's my left not your

07:45

litter you guys I left and then the last

07:48

thing is reducing size of the container

07:50

now this only applies with things with

07:52

gases in them and you basically compare

07:54

the right side number of gas molecules

07:56

on the left side number of gas molecules

07:58

so every dude is the container size

07:59

right each molecule of gas takes up

08:01

certain amount of space so if you want

08:02

to counteract the change over getting a

08:04

smaller container you also want to

08:05

reduce the size of the gas molecule and

08:07

in order to do that you just want to

08:08

reduce the number of gas molecules

08:09

overall so if you reduce the container

08:11

size you want to move to the side that

08:13

has less gas molecules and in this case

08:15

that's the right so your reaction gonna

08:17

move right ok very epic battle a champ

08:19

let's talk about the last important

08:20

thing determining rate laws all right

08:22

he's getting it every problem I found

08:24

off the internet and it basically gives

08:26

you a bunch of rate laws and I want you

08:28

to find the overall rate law of the

08:29

reaction so my favorite way to approach

08:30

this problem and just a right

08:32

many acquainted as you can of course the

08:34

first thing I don't recognize it wants

08:36

the rate-determining step that's right

08:37

the slow step because everything gonna

08:39

get traffic jammed at the slow step

08:41

because that guy is hanging long this is

08:43

like if you're running in line right the

08:44

fast guy they're gonna run but then the

08:46

guys behind the slowlier is gonna get

08:47

stuck with your water I don't know how

08:48

is analogies going but he gets ideas the

08:50

slow step is the rate determining step

08:51

it's the front guy is slow everybody

08:53

below behind it was gonna be slow so

08:55

essentially it's the rate of the overall

08:57

reaction is that the rate of the slow

08:58

step and when you're given elementary

09:00

stuff you're allowed to you the

09:01

coefficient to determine the rate law so

09:03

in this case the rate law right now is

09:06

kate no.2 no.3 however our actual

09:10

reaction doesn't have any no.3 in it so

09:13

like this rate law doesn't really make

09:16

much sense because we shouldn't have to

09:17

know about intermediates in order to

09:19

determine the rate law of an overall

09:21

reaction so we somehow to get rid of

09:22

this no.3

09:23

so where can we write equated well we

09:25

can't write any equation for kinetics

09:27

the Koch kinetics is purely expressions

09:29

you can't write any equation so what do

09:31

we have to write equation for that's

09:32

right equilibrium that's why your time

09:33

but you can leave me today get it ha ha

09:35

no I don't know what I'm saying so

09:36

basically if we write the equilibrium

09:38

expression basically you know the

09:40

forward rate is equal to the backward so

09:42

k1 and 205 is equal to K negative 1 no.2

09:49

and no.3 now all I have to do is just

09:52

ignore all the case ok we don't care

09:54

about cave because eventually they'll

09:56

all just like be they'll be some random

09:58

like k 1 over k 1 negative 1 over K

10:00

times K times there's another key 3

10:02

times k2 but we don't care because that

10:04

all could just be written out of a

10:05

single k we could say that this new KK

10:08

prime that we made up is equal to all

10:10

the other case so if we can just ignore

10:11

them so we have no.2 no.3 here we have n

10:15

2 O 5 here and we want to get rid of the

10:17

no.3 but we could literally just plug in

10:20

the n2o5 for no.2 times and the 3 and we

10:23

get that our rate lock is equal to into

10:25

a 5 but don't forget we have to put back

10:28

or case so let's put our k and boot we

10:30

got a rate lon let's say for example

10:31

that this over here with the 2 right

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then this over here would be n of 2

10:35

squared + 2 a 5 squared and then this

10:38

over here would be into a 5 squared as

10:40

well so that is how you do rate lon you

10:44

first

10:45

look at the slow stuff and set its rate

10:47

to the overall rate okay so you got that

10:49

then you look at the equilibrium step

10:51

and you're riding the quake and then

10:52

once you get to equation you want to see

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what's in the reactant side and you want

10:56

to get rid of anything that's not on the

10:58

reactant side but you can substitution

10:59

eliminate whatever it's added do you

11:01

want and you only have two things to

11:02

worry about your expression that you got

11:04

from the rate determining step and your

11:06

equilibrium equation alright very happy

11:09

that's all I got to talk about if you

11:10

got one more of these transporters just

11:12

let me know as always if you enjoyed the

11:14

video leave a like and subscribe for

11:15

more hope it was helpful thing up for

11:17

watching again see you guys the next

11:18

time