Final answer:
The amount of energy released during a reaction is related to the reaction's thermodynamics but does not determine the rate of the reaction, which is influenced by kinetic factors such as activation energy.
Step-by-step explanation:
The statement 'The amount of energy released during a reaction tells nothing about the rate at which that reaction will occur' is true. The energy change associated with a chemical reaction is related to the thermodynamics of the reaction and tells us whether a reaction is energetically favorable or not. However, the reaction rate is determined by kinetic factors, specifically the activation energy which is the energy required to initiate the reaction, and the presence of a catalyst.
For example, some reactions can release a large amount of energy but may occur very slowly because they have high activation energy barriers that molecules must overcome to react. Conversely, other reactions may have low energy release but proceed rapidly if they have low activation barriers or are catalyzed efficiently.