Please could you look at question Q3)b)iii).... the mechanism one. I do not understand the mark scheme. Why is it that only one molecule is needed when in the equation in the question, it states something else?
Please could you look at question Q3)b)iii).... the mechanism one. I do not understand the mark scheme. Why is it that only one molecule is needed when in the equation in the question, it states something else?
The rate equation gives you the molecules that are in the rate determining step - you can see the concentration of N2O5 is raised to the first power meaning there is only one molecule of this present in the rate determining step - it can't be mechanism B because there are 2 molecules of N2O5
The rate equation gives you the molecules that are in the rate determining step - you can see the concentration of N2O5 is raised to the first power meaning there is only one molecule of this present in the rate determining step - it can't be mechanism B because there are 2 molecules of N2O5
It's because the rate equation is first order with respect to N2O5, mechanism B (two molecules) is second order.
But I thought that since the rate equation has the N2O5 raised to first order.. it just means that the concentration is directly proportional to the rate. Also I thought that you can determine the reaction order only experimentally. Isn't it the power next to the square bracktets which is used to show the coeeficient only used in equilirbria constants?
But I thought that since the rate equation has the N2O5 raised to first order.. it just means that the concentration is directly proportional to the rate. Also I thought that you can determine the reaction order only experimentally. Isn't it the power next to the square bracktets which is used to show the coeeficient only used in equilirbria constants?
No, the power to which the concentration is raised also gives the number of molecules of the reactant in the rate determining step
Also I thought that you can determine the reaction order only experimentally.
This is true, but the rate equation gives you information about the mechanism There are several steps in many chemical reactions and you don't know which is rate limiting until you've done some experimentation
So given this, you can make a rate equation just by looking at the coefficients of the reactants?
This is true, but the rate equation gives you information about the mechanism There are several steps in many chemical reactions and you don't know which is rate limiting until you've done some experimentation
No
Rigghhtt.. so if I could just clear this from my head. If you were given an equation of a reaction like 2N2O5 ----> 4NO2 + O2 you will do experiments and see how the concentration of the N2O5 will effect the rate. And you find out that Rate = k[N2O5]^1. Then you wish to know the mechanism. So you would know that the Overall rate = the rate of the rate determininbg step (rds). So the rds involves only the N2O5.
If I rate equation had [2N2O5] then would this mean that the mechanism also involves 2N2O5?
Rigghhtt.. so if I could just clear this from my head. If you were given an equation of a reaction like 2N2O5 ----> 4NO2 + O2 you will do experiments and see how the concentration of the N2O5 will effect the rate. And you find out that Rate = k[N2O5]^1. Then you wish to know the mechanism. So you would know that the Overall rate = the rate of the rate determininbg step (rds). So the rds involves only the N2O5.
This is correct
If I rate equation had [2N2O5] then would this mean that the mechanism also involves 2N2O5?
Ahh.. I get it... is this just something we have to remember or there is a reason for this?
There is always a reason
If you have a reaction that goes A + B ---> C in a single step then the rate of the reaction is written: rate = k[A][B] which I'm sure you're familiar with
Compare this with a single step reaction A + A --> D then you would write this rate as: rate = k[A][A] or rate = k[A]2 since there are two molecules of A involved.
[QUOTE="EierVonSatan;41962061"]There is always a reason
If you have a reaction that goes A + B ---> C in a single step then the rate of the reaction is written: rate = k[A] which I'm sure you're familiar with
Compare this with a single step reaction A + A --> D then you would write this rate as: rate = k[A][A] or rate = k[A]2 since there are two molecules of A involved.
Hoes that help?
Yeah.. I get it. Thanks
I just stumbled upon another question which is pretty easy but yet again strange.
I understand the order of reaction wrt O3 BUT I don't get the ethene order. I used the last two experiments with ethene so that the 2/1 = 2 and when I did same with the rate.. I found 16/4 = 4. So clearly the rate of the reaction is square of the concentration of ethene. Therefore the order is 2. So why does it say 1 in the MS?
I just stumbled upon another question which is pretty easy but yet again strange.
I understand the order of reaction wrt O3 BUT I don't get the ethene order. I used the last two experiments with ethene so that the 2/1 = 2 and when I did same with the rate.. I found 16/4 = 4. So clearly the rate of the reaction is square of the concentration of ethene. Therefore the order is 2. So why does it say 1 in the MS?
Imagine that experiment 3 had an ethene concentration of 1.0 what would you expect the rate to be, knowing the order with respect to ozone?
Compare this value with experiment 3, what is the order for ethene?