Collision Theory - Arrhenius Equation & Activation Energy - Chemical Kinetics - By The Organic Chemistry Tutor
Transcript
00:00 | in this tutorial let's talk about the collision theory model | |
00:05 | . So what's the basic idea behind the collision theory | |
00:09 | ? The basic idea is that from molecules to react | |
00:12 | they have to collide if they don't collide , there's | |
00:16 | not gonna be any chemical reaction . If there's no | |
00:19 | physical contact between these molecules , nothing's going to happen | |
00:22 | . So molecules must collide in order to react . | |
00:26 | The second thing is they have to have the correct | |
00:29 | molecular orientation in order for a reaction to proceed . | |
00:34 | So to illustrate this , let's say if we have | |
00:38 | hydroxide and hydroxide is going to react with methyl bromide | |
00:46 | . Ch three br now bro ming is more electoral | |
00:51 | negative than carbon . So it bears a partial negative | |
00:54 | charge and carbon is less electric negative than grooming . | |
00:58 | So it's partially positive . The element that's more electro | |
01:02 | negative is gonna pull the electrons toward itself . And | |
01:05 | that's why brahman has the partial negative charge . So | |
01:08 | , hydroxide , since it has a negative charge , | |
01:12 | it's attracted to the carbon in methyl bromide . So | |
01:15 | it wants to attack this carbon does expelling the bromide | |
01:19 | ion and so this will create methanol . So if | |
01:23 | it approaches from the back of the methyl bromide , | |
01:27 | if it attacks from the carbon side , it has | |
01:30 | the correct molecular orientation . So the reaction is going | |
01:33 | to work . Now let's say if it approaches it | |
01:36 | from the other direction . So let's say this is | |
01:39 | methyl bromide and hydroxide is coming in this direction . | |
01:44 | Well , the reaction is not going to happen . | |
01:47 | Hydroxide is repelled by the partial negative charge of the | |
01:51 | bromine atom . And so when two negative charges come | |
01:54 | together , they're going to fill a force that's going | |
01:57 | to repel them . And so that's going to prevent | |
02:00 | the reaction from occurring . Whereas when hydroxide attacks from | |
02:04 | the carbon side , the negative charge on the hydroxide | |
02:08 | is attracted to the partial positive charge on the carbon | |
02:11 | atom and that electrostatic force of attraction accelerates them together | |
02:16 | , which favors the collision of those two molecules . | |
02:20 | And so if the two molecules do not have the | |
02:22 | correct molecular orientation , the reaction is not going to | |
02:26 | happen , but if they collide with the appropriate orientation | |
02:31 | , then the reaction is going to happen . So | |
02:34 | in order for a reaction to occur , molecules , | |
02:36 | they have to collide and two , they have to | |
02:39 | collide with the right orientation . Now , the third | |
02:42 | thing is that they need enough energy because if the | |
02:46 | temperature is low , even though these two may be | |
02:49 | attracted to each other , if the hydroxyurea and doesn't | |
02:52 | move with enough momentum , it's not going to be | |
02:55 | enough to knock off this bromide ion , so it | |
02:58 | has to have enough energy to attack the carbon atom | |
03:02 | and expel the bromine iron out of that reaction to | |
03:05 | create methadone . So there's three things that is required | |
03:11 | for a reaction to take place . The molecules must | |
03:13 | collide and they have to collide with the right orientation | |
03:16 | and they have to have sufficient energy . Two break | |
03:21 | some bonds and form some new bonds . Now this | |
03:26 | leads us into energy diagrams . So on the Y | |
03:30 | axis is the energy of the system , on the | |
03:33 | X axis is going to be the reaction coordinate . | |
03:39 | Mhm . Here we have the reactant and here we | |
03:42 | have the products . The top is the transition state | |
03:46 | , also known as the activated complex . In order | |
03:49 | for this reaction to occur , the system has to | |
03:53 | have enough energy the reactions need to gain of energy | |
04:00 | . There's something called activation energy , which is the | |
04:03 | difference between the energy of the transition state and the | |
04:06 | energy of the react . It's if the reactant do | |
04:10 | not have enough energy to overcome the activation energy , | |
04:13 | the reaction will not happen . So if they can't | |
04:17 | get above this hill , there's no reaction that's going | |
04:21 | to take place . So they have to have enough | |
04:23 | energy to get over that hill . And so that | |
04:26 | minimum energy to get the reaction started as the activation | |
04:29 | energy . So even if a molecule collides with the | |
04:32 | right orientation , if they don't have enough energy to | |
04:36 | make it to the activated complex , then the reaction | |
04:39 | is just not going to happen . So one way | |
04:42 | you can get up there is by increasing the temperature | |
04:44 | . Whenever you increase the temperature , the rate of | |
04:46 | the reaction increases the fraction of molecules that can reach | |
04:52 | the activate complex will increase . Now one thing I | |
04:56 | want to specify is this is known as the forward | |
04:59 | activation energy . There's something called the reverse activation energy | |
05:04 | , which is the energy difference between the products and | |
05:07 | the transition state . So in this example , it's | |
05:10 | easier to go this way then to go that way | |
05:18 | . Now the next thing you need to know is | |
05:19 | that notice that the difference between the energy of the | |
05:22 | products is greater than the energy of the reactions . | |
05:25 | Whenever the energy of the products is greater than the | |
05:27 | reactant , what you have is an end a thermic | |
05:29 | reaction . In order for this reaction to occur , | |
05:33 | energy has to be put into the system . An | |
05:36 | extra thermic reaction looks like this . The energy of | |
05:39 | the reactant is going to be greater than the energy | |
05:42 | of the products . So this is an exotic reaction | |
05:49 | . Now , initially you gotta put in energy to | |
05:52 | get to the activated complex to get the reaction started | |
05:55 | . Once you overcome that barrier , then a lot | |
05:58 | of energy is gonna be released . So you got | |
06:00 | to put in a small amount of energy to get | |
06:02 | started but you're gonna get a large amount of energy | |
06:04 | once the process is started . And so that's a | |
06:07 | an extra thermic reaction . Now let's talk about the | |
06:11 | Iranians equation K . Is equal to ZP E . | |
06:18 | Raised to the negative E . A . Over artie | |
06:23 | . Now see is known as the collision frequency . | |
06:28 | If you can increase the collision frequency of reaction , | |
06:31 | the rate of the entire reaction will go up . | |
06:35 | P is hysteric factor and this has to do with | |
06:45 | The fraction of collisions that have the right orientation . | |
06:48 | So this is a number between zero and 1 and | |
06:52 | it depends on the nature of the reactant . Now | |
06:59 | this part E , which is the inverse of the | |
07:03 | natural log function , raised to the negative Ea over | |
07:05 | RT . That represents the fraction of molecules that have | |
07:09 | sufficient energy to get the reaction going . So notice | |
07:13 | that it depends on temperature and activation energy . So | |
07:17 | if you want a reaction to occur , there's two | |
07:19 | things you can do to help it to make it | |
07:22 | work . You can increase the temperature and that can | |
07:25 | give the molecules the energy they need to overcome that | |
07:28 | barrier . As you increase the temperature , the rate | |
07:31 | of the reaction will increase . The second thing you | |
07:34 | could do is add a catalyst . Whenever you add | |
07:36 | a catalyst . A catalyst provides an alternative pathway for | |
07:40 | the reaction and by doing so it lowers the activation | |
07:43 | energy , which increases the rate of the reaction . | |
07:49 | Now , the last thing when you talk about is | |
07:52 | the product cp Z . P is equal to aim | |
07:56 | , which is also known as the frequency factor , | |
07:59 | is the product of the collision frequency and hysteric factor | |
08:07 | . So now let's put this all together . Now | |
08:11 | let's consider a first order reaction . Where we have | |
08:15 | rate is equal to the rate constant Kane times the | |
08:20 | concentration of A . And we know that the rate | |
08:25 | constant K . Is equal to the frequency factor times | |
08:31 | E . Raised the negative E . A . Over | |
08:34 | artie . And the frequency factor can be replaced with | |
08:39 | the collision frequency times hysteric factor and then times this | |
08:47 | . So Z . The collision frequency represents the total | |
08:52 | number of collisions per second . That's a current in | |
08:55 | the reaction . P The hysteric factor which we said | |
08:59 | was between zero and 1 . That's the fraction of | |
09:03 | molecules with the proper orientation . Or more specifically , | |
09:08 | that's the fraction of collisions that are occurring with the | |
09:12 | proper orientation . So you can think of PS the | |
09:15 | probability that two molecules will collide with the right orientation | |
09:22 | . This portion here which we describe as the fraction | |
09:25 | of collisions with sufficient energy . You could also think | |
09:29 | of it as the probability that two molecules that are | |
09:32 | colliding will have enough energy to overcome the activation barrier | |
09:38 | . So you can think of these two values as | |
09:40 | probabilities or fractions . So is the is the collision | |
09:46 | frequency and P . Is the probability that tomb colliding | |
09:51 | molecules will have the right orientation . A represents the | |
09:55 | total number of collisions per second that's occurring . Interview | |
09:59 | action with the right orientation . Now , if we | |
10:04 | multiply the frequency factor by the fraction of molecules having | |
10:09 | sufficient energy , we can dust come up with an | |
10:13 | understanding of the very constant K . So we can | |
10:15 | say that the rate constant K . Represents the total | |
10:19 | number of collisions per second having the proper molecular orientation | |
10:24 | , as well as sufficient energy needed to overcome the | |
10:29 | activation energy barrier to get the reaction going to convert | |
10:33 | the reactions into products . So the very constant K | |
10:37 | . Takes all of those factors into account . Now | |
10:43 | , let's talk about what happens when we increase the | |
10:47 | concentration of the reaction . A as we increase the | |
10:51 | concentration of the reactant , there's gonna be more collisions | |
10:55 | . The number of collisions will increase and therefore the | |
11:00 | rate of the reaction will increase . Now what about | |
11:04 | if we increase the temperature , if we increase the | |
11:07 | temperature , the average kinetic energy of the molecules will | |
11:12 | increase . So molecules are going to be moving faster | |
11:16 | , the molecular speed of the molecules will increase as | |
11:19 | well . And therefore there's gonna be more collisions . | |
11:24 | And this too will increase the rate of the reaction | |
11:29 | . Now you can think about it another way to | |
11:31 | and this formula , the temperature affects the re constantly | |
11:36 | . Now the temperature is in the bottom of the | |
11:38 | fraction and typically when you increase the denominated refraction , | |
11:44 | the value of the fraction goes down . However , | |
11:48 | notice that we have a negative exponents . And so | |
11:54 | because of that , when you increase the temperature it | |
11:58 | has the effect of increasing K . It's like a | |
12:01 | double negative . You can think of it that way | |
12:03 | . When you increase the temperature , the rate constant | |
12:06 | K goes up , the fraction of molecules having sufficient | |
12:10 | energy to overcome the activation barrier increases . And when | |
12:16 | K goes up , the rate constant goes up as | |
12:20 | well . And let's show this with a distribution proof | |
12:34 | . So we're going to have energy on the X | |
12:37 | axis and we're going to have the number of molecules | |
12:45 | on the y axis . It's not moles but molecules | |
12:50 | . And we're gonna have two curves , one at | |
12:53 | a lower temperature which will say look something like this | |
12:57 | , and another curve which I'll drawn blue at a | |
13:01 | higher temperature . So this one will be , let's | |
13:09 | say at a temperature of 300 Kelvin And the other | |
13:12 | one will be at a higher temperature will say at | |
13:14 | 500 Calvin And somewhere along the X axis we're going | |
13:20 | to have E . A . The activation energy . | |
13:27 | So anything above E . A . Represents the fraction | |
13:31 | of molecules have in sufficient energy , sufficient collision energy | |
13:36 | , so to speak enough so that they can overcome | |
13:40 | the energy barrier to make the reaction going . And | |
13:45 | let's put that in green . So in green , | |
13:52 | that represents the fraction of molecules at 300 Calvin , | |
13:55 | having enough energy to make the reaction go . But | |
13:59 | in red , which encompasses the area in green as | |
14:04 | well , that represents the fraction of molecules have enough | |
14:07 | energy to overcome the energy barrier to also make the | |
14:11 | reaction work . But notice that at 500 Calvin the | |
14:16 | fraction of molecules that have enough energy is greater . | |
14:20 | Then the fracture of molecules that 300 Kelvin is significantly | |
14:23 | greater . And so that's what happens when you increase | |
14:27 | the temperature . When you increase the temperature , the | |
14:30 | average kinetic energy of the molecules go up . So | |
14:32 | therefore the fraction of molecules have enough energy to make | |
14:38 | the reaction go , and that fraction increases . And | |
14:43 | so if more molecules have more energy , two get | |
14:47 | the reaction go on . The overall rate of the | |
14:49 | reaction will increase . Now let's talk about what's going | |
14:55 | to happen if we were to add a catalyst to | |
15:00 | the reaction , what do you think is going to | |
15:02 | happen if we introduce the catalysts ? A catalyst has | |
15:09 | the effect of lowering the activation energy . Now , | |
15:16 | here's a visual description of that . So this is | |
15:21 | a potential energy diagram . We have potential energy on | |
15:25 | the Y axis and the progress of the reaction on | |
15:29 | the X axis . So let's say we have something | |
15:35 | that looks like this , where this represents the energy | |
15:38 | of the reactant since the products . And this is | |
15:41 | the transition state . For a catalyzed reaction , it | |
15:48 | would look something like this . So this is the | |
15:55 | un catalyzed reaction and this is the catalyzed reaction . | |
16:09 | The activation energy is the difference between the energy of | |
16:11 | the reactant and the transition state . But notice that | |
16:16 | when you add a catalyst , the activation energy decreases | |
16:23 | , a catalyst achieves this by providing a reaction with | |
16:28 | an alternative pathway . It actually changes the reaction mechanism | |
16:34 | . It allows the reactant to become products using by | |
16:39 | taking a different route , so to speak . So | |
16:42 | that's how the catalysts can lower the activation energy . | |
16:46 | It helps the reaction find an easier way to go | |
16:49 | from reactions to products . Now notice that activation energy | |
16:55 | is in the numerator of that exponential fraction . West | |
16:59 | temperature is in the denominator . Now we know that | |
17:04 | an increase in temperature leads to an increase in the | |
17:09 | very constant K . So what happens if we increase | |
17:15 | the activation energy ? Well it should have the opposite | |
17:19 | effect . It should decrease K . T . Is | |
17:25 | in the denominator E . A . S . In | |
17:27 | the numerator . So if increase in T . Leads | |
17:30 | to an increase in K . Increase in E . | |
17:33 | A . Will decrease Kane . Likewise the reverse is | |
17:36 | true . If we decrease the activation energy the very | |
17:40 | constant case should go up and that's what happens when | |
17:44 | you add a catalyst , the activation energy goes down | |
17:47 | , the rate cost and go the red costing K | |
17:50 | . Goes up . And so the overall rate of | |
17:52 | the reaction increases . So those are some ways in | |
17:57 | which you can increase the rate of a chemical reaction | |
18:01 | . So to summarize if we increase the concentration of | |
18:04 | the reacted , the rate is gonna go up . | |
18:08 | If we increase the temperature , the rate of the | |
18:11 | chemical reaction will go up and if we add a | |
18:14 | catalyst the activation energy will go down and the rate | |
18:19 | of the reaction will go up . So those are | |
18:22 | some different ways in which we can increase the rate | |
18:25 | of a chemical reaction . You can increase concentration , | |
18:28 | raise the temperature or introduce the catalysts to speed up | |
18:32 | the reaction . Now , let's write down some equations | |
18:36 | that you need to know in order to solve problems | |
18:39 | . So you're already familiar with this one . The | |
18:41 | rate constant K . Is equal to the frequency factor | |
18:45 | times E . Race to the negative E . A | |
18:49 | . Over artie . Here's another one that you should | |
18:53 | be familiar with . The natural log of the very | |
18:57 | constant K . That's equal to negative E . A | |
19:04 | . Over our times . One over T . Plus | |
19:10 | the natural log of ain . Now , in this | |
19:17 | form , this is written in slope intercept form . | |
19:22 | So why corresponds to Ellen K . The slope M | |
19:26 | corresponds to negative E . A . Of art X | |
19:30 | corresponds to one of the T . And the Y | |
19:33 | intercept B . Is Ellen A . So if you | |
19:38 | were to graph why versus X . Where why is | |
19:43 | Ellen K . So we'll put that on the X | |
19:45 | axis , I mean the Y axis and one of | |
19:49 | the T . S . X . So we'll put | |
19:50 | one of the T . On the X axis . | |
19:56 | You're gonna get a graph that looks like this . | |
19:58 | It's going to be a straight line plot . But | |
20:00 | notice that the slope is negative . So the slope | |
20:05 | of this line is going to equal negative E . | |
20:09 | A . Over our and the Y intercept which this | |
20:15 | is where the graph starts from . That's going to | |
20:19 | be Ln . A . So for problems associated with | |
20:25 | this equation , if you have a plot of Ellen | |
20:27 | K versus one of the T . Just know that | |
20:30 | you can find the activation energy from the slope of | |
20:33 | the graph . And the white intercept Is equal to | |
20:39 | the natural log of eight . So you could find | |
20:41 | a frequency factor from the Y intercept . Now are | |
20:47 | is 8.3145 jules Permal per Calvin . So because our | |
20:54 | has the jewels and moles . The activation energy which | |
20:59 | is typically reported in colleges promote when you use it | |
21:02 | in these formless , it needs to be in jules | |
21:05 | promote , so you need to convert so when reporting | |
21:10 | the activation energy you want your answer to the intelligence | |
21:13 | promote . But whenever you plug it into one of | |
21:15 | these formulas you need to convert it to jules promote | |
21:18 | . So make sure to be aware of that . | |
21:21 | Yeah , now the smoke em is equal to negative | |
21:25 | E . A . Over our . And the slope | |
21:29 | is why two minus Y . One Divided by X | |
21:33 | 2 - . Excellent . Ellen K . Is on | |
21:36 | the Y axis . One of her T . Is | |
21:38 | on the X axis . So if Y is equal | |
21:41 | to Ellen K . We could say that this is | |
21:43 | Ellen K two - Ellen K one all divided by | |
21:49 | one over T two -1 over T . one . | |
21:54 | So that's going to equal negative E . A . | |
21:57 | Over our . Now let's see if we have L | |
22:00 | N A minus L N B . Using the property | |
22:03 | of natural logs or logs , we can convert this | |
22:06 | into a single log expression by writing it like this | |
22:10 | . Ellen A over B . So we can write | |
22:13 | this as a single long expression as well . We | |
22:15 | can say that that's LNA . I mean that's Ellen | |
22:18 | K two over K one And this is one over | |
22:25 | T 2 -1 over team one . Mhm . And | |
22:30 | that equals negative E . A . Over our . | |
22:35 | Now if we want to get activation energy by itself | |
22:39 | we can multiply both sides by negative art . If | |
22:45 | we do that our will cancel on the right side | |
22:48 | as well as the negative sign . Mhm . And | |
22:51 | we'll get an equation for activation energy . So the | |
22:57 | activation energy is gonna be negative art . Ellen K | |
23:03 | two over K . one Divided by one over T | |
23:09 | 2 -1 of the T . one . So you | |
23:12 | could use this equation to calculate activation energy . Now | |
23:16 | you might see a variant of this equation . Sometimes | |
23:19 | this negative sign will be distributed to one of the | |
23:22 | T . Too modest one of the T . One | |
23:24 | and that will basically flip The order of T . | |
23:27 | one and T . two . So this is also | |
23:28 | equal to positive art . Ellen K two overcame run | |
23:34 | . And if you distribute the negative sign negative times | |
23:37 | negative one of the T becomes positive for one of | |
23:40 | the T . One . And then here this will | |
23:42 | be negative So -1 of the T . two . | |
23:46 | So you might see in that format to so just | |
23:49 | be aware of that . But if you have the | |
23:50 | negative sign it's going to be one of the T | |
23:52 | . Two minus one of the T . One instead | |
23:55 | of the reverse . Now let's go back to this | |
23:59 | equation . Mhm . Make sure to write this equation | |
24:03 | by the way because you're gonna need it to solve | |
24:05 | problems . Now instead of multiplying both sides by negative | |
24:26 | art , let's multiply both sides by this term . | |
24:31 | If we do that we'll get a different equation we'll | |
24:37 | get this one Ln K two Divided by K . | |
24:43 | one is equal to negative E . A . Over | |
24:50 | our . And we're going to move this to the | |
24:52 | other side , Times one over T two -1 over | |
24:57 | T . one . So that's another form of the | |
25:02 | Iranians equation that you might see it in . Now | |
25:08 | what we're gonna do at this point is we're gonna | |
25:10 | put both sides of this equation on the exponents of | |
25:15 | E . So I'm gonna put all of this on | |
25:20 | the exponents of E . And all of this on | |
25:24 | the X . Point of E . Because he is | |
25:28 | the same and these two are equal to each other | |
25:32 | . Both sides of this equation will be equivalent now | |
25:35 | the base of a natural log Izzy . So on | |
25:37 | the left side These two will cancel . And so | |
25:42 | we're just gonna get K . two over K1 is | |
25:45 | equal to everything that we see here . Now if | |
25:50 | we multiply both sides by K . one We can | |
25:54 | get an expression for K . two . So you | |
25:57 | want to write down this formula because sometimes you need | |
25:59 | to calculate a new very constant at a new temperature | |
26:03 | . So that new rate constant K two is equal | |
26:05 | to K . One times E . Raised to the | |
26:09 | negative E . A . Over our Times one over | |
26:12 | T 2 -1 of the T . one . So | |
26:17 | this is the second equation that you want to write | |
26:18 | down . So you have an equation that will help | |
26:21 | you to calculate the activation energy . And this equation | |
26:24 | will help you to calculate the new very constant given | |
26:28 | a new temperature . Now let's go back to the | |
26:36 | equation that we started with on this screen . All | |
26:43 | right . That's as far as uh my software will | |
26:46 | let me go back . Now sometimes you need to | |
26:56 | calculate the second temperature . So what we're gonna do | |
26:59 | is we're gonna isolate T . two to do that | |
27:02 | . We're going to multiply both sides by negative are | |
27:05 | over E . A . So those will cancel we're | |
27:17 | going to have negative art . Ellen K two Divided | |
27:24 | by K . one over E . A . That's | |
27:27 | going to equal one over T 2 -1 over T | |
27:30 | one . So we're going to move this to the | |
27:32 | other side where it will become positive . So we | |
27:36 | have run over T1 minus R . Ellen K . | |
27:42 | two over K . one Overeat eh That's equal to | |
27:46 | one over T . two . That we're going to | |
27:49 | raise both sides to -1 . One of the T | |
27:53 | two . Raised to the negative one power is just | |
27:55 | T . Two . So we get this equation T | |
27:57 | two is equal to one over T . One minus | |
28:02 | R . Ellen K two Overcame 1 . Overeat eh | |
28:09 | And this is raised to the -1 power . So | |
28:13 | this will help you to calculate the second temperature if | |
28:16 | you know the secondary constant . And if you know | |
28:19 | the activation energy . So those are some formulas that | |
28:22 | you want to use when solving problems associated with the | |
28:27 | Iranians equation , activation energy , very constant and things | |
28:30 | like that . Now let's go ahead and put these | |
28:33 | equations to good use . So we're gonna work on | |
28:36 | a few practice problems . So take this one for | |
28:40 | example , A certain reaction has an activation energy of | |
28:43 | 50 killer juice promotes The rate constant at 25°C is | |
28:48 | .0039 Minutes to the -1 . What is the value | |
28:53 | of the rate constant ? At 75°C. . So first | |
28:59 | let's make a list of what we know . So | |
29:02 | we have the activation energy . It's 50 kg , | |
29:05 | promote The rate constant which will call K . one | |
29:10 | is .0039 . And that's why the temperature of 25°C, | |
29:16 | , which we need to convert to Kelvin . So | |
29:19 | add 73-25 . That gives you 2 98 Kelvin . | |
29:23 | Mhm . Our goal is to calculate K tune And | |
29:27 | the second temperature is 75 plus 2 73 . So | |
29:31 | that's 348 Calvin . So what is the formula that | |
29:35 | will help us to calculate K . 2 ? It's | |
29:40 | K . two is equal to K . one times | |
29:43 | E . Raised to the negative E . A . | |
29:46 | Over our Multiplied by one over T two -1 over | |
29:51 | T . one . So any time you need to | |
29:56 | find a very constant at a different temperature . That's | |
30:00 | the formula that you want to commit to memory . | |
30:03 | Now came one we know 2.0039 . The activation energy | |
30:08 | has to be in jewels . So we got to | |
30:11 | multiply 50 by 1000 . So it's gonna be 50,000 | |
30:15 | and then it's one over T . Two which is | |
30:17 | 348 -1 over T . one which is 2 98 | |
30:22 | . And then divide that by our Our is 8.3145 | |
30:27 | jules promote per Calvin . You don't want to use | |
30:30 | the gas constant for our .0826 . It's not going | |
30:34 | to work for this equation . So if you type | |
30:46 | this entire thing the way you see it , what | |
30:50 | you doing one step at a time , you should | |
30:52 | get this answer . K two is .0708 . So | |
30:59 | notice that K two is greater than K one .07 | |
31:04 | is greater than .003 . Now this answer makes sense | |
31:08 | because the second temperature is higher than the first temperature | |
31:13 | . And as you increase the temperature of a reaction | |
31:18 | , the rate constant will increase . When the rate | |
31:20 | constant goes up , the rate of the chemical reaction | |
31:23 | will go up as well . And so that's it | |
31:26 | for this problem . |
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