The hydrogenation reaction is an exothermic reaction; why then does increasing the temperature facilitate its progress?
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The book says that from a dynamic perspective, raising the temperature is more beneficial for the reaction; I don’t understand it.
The hydrogenation reaction is an exothermic reaction; increasing the temperature is unfavorable for the chemical equilibrium of hydrogenation, but it is beneficial for dehydrogenation and cracking reactions. Within a certain temperature range, increasing the temperature can accelerate the reaction rate. For different raw materials, the reaction activation energy varies; consequently, the increase in reaction rate upon raising the temperature also differs. The higher the activation energy, the faster the reaction rate increases when the temperature is raised.
Increasing the reaction temperature within a certain range enhances the reaction depth, improves the conversion rate, and is beneficial for hydrogenation reactions
This is the activation energy required during a chemical reaction. Below a certain temperature, this reaction does not occur. So heat must be supplied to drive its reaction.
The hydrogenation reaction is an exothermic reaction; from a thermodynamic perspective, increasing the temperature is not conducive to the progress of the reaction. From a kinetic perspective, increasing the temperature accelerates the reaction rate and shortens the reaction time, which is beneficial for the progress of the reaction.
The hydrogenation reaction is an exothermic reaction, so increasing the temperature certainly does not favor its forward progression. However, this statement is correct in that the forward progression is based on the reaction equilibrium point. In most chemical reactions, the reaction does not reach equilibrium (since it takes too long for most reactions to reach equilibrium, incomplete reactions are usually used, followed by multiple rounds of the reaction). Therefore, increasing the temperature appropriately can speed up the reaction, allowing it to proceed more rapidly and even reach equilibrium (at which point the equilibrium point shifts to the left).
Increasing the reaction temperature increases the reaction rate.
Increasing the temperature can reduce the reaction activation energy and increase the probability of molecular collisions
Raising the temperature reduces the energy required to activate molecules, making reactions easier to occur.