URGENT Chemistry Question: Which of the Statements is Correct?

[beocom6000yello]

URGENT QUESTION: Chemistry

i would think that enthalpy of reaction would always have to be greater than activation in order to proceed. however, i thought the rest were false.

please help me...this is very frustrating.


This problem involves consideration of the following statements.

(a) Slow reactions have more elementary steps than fast reactions.
(b) The slowest step comes last in a reaction mechanism.
(c) The slowest step comes first in a reaction mechanism.
(d) Fast reactions have fewer elementary steps than slow reactions.
(e) Fast reactions have only one elementary step.
(f) Enthalpy of reaction is larger than activation energy.
(g) Enthalpy of reaction is smaller than activation energy.

Which of the following combinations of the above statements is correct?

all are correct

none is correct

(a), (c), and (f) are correct

(e) is correct

(d) and (f) are correct

(a) is correct

(b), (e), and (f) are correct

 

[Kushal]

the more intermediate steps you have in a reaction, the slower this reaction will be.

 

[Blueshift5]

The correct combination of statements is (a), (c), and (f). This is because slow reactions do have more elementary steps than fast reactions, and the slowest step does come first in the reaction mechanism. Additionally, the enthalpy of reaction is always larger than the activation energy in order for a reaction to proceed. It is important to note that while (f) is correct, it does not necessarily mean that (g) is incorrect. Both statements can be true in different scenarios.