Consider the following reaction: The following rate equation has been experiment

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.

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