Consider the following reaction: The following rate equation has been experiment
ID: 711585 • Letter: C
Question
Consider the following reaction:The following rate equation has been experimentally established for this process: Rate = k[HO-][CH3CH2Br]
The energy diagram for this process is shown below: Integrated Problem 06.42b Consider the folowing reaction: H,C H, The following rate equation has been experimentally established for this process The energy diagram for this process is shomn below: Free energy HO -Br Reaction coordinate Would you expect this process to be exothermic or endethermic? Explain A CHyCH2-Br is broken, and a CHjCH2-OH is formed. AH for this reaction is expected to be L which means that the reaction should be
Explanation / Answer
Ans) The process is an exothermic process.
Change in H is negetive and hence the reaction should be exothermic.
The free energy coordinate shows that the products have a lower free energy than that of the reactants.
So, change in free energy(delta G) for this process is negetive.
Now, delta G = delta H - T(delta S)
This reaction has no change in number of molecules that is there are same number of molecules in the product as the reactants. So, delta S = 0
This makes delta H also to be negetive and so is verified by the reaction as it is exothermic.
The reaction is a second order reaction since the rate equation is rate = k[OH-][CH3CH2Br]. The coefficients of OH- and CH3CH2Br add to be 2. So this makes the order of the reaction to be 2.