Which of the following correctly describe an exergonic reaction? Select True or False for each statement. T/F The products have lower Gibbs free energy than the reactants. T/F Activation energy is required for the reaction to proceed. T/F The products always have lower entropy than the reactants. T/F The reaction always occurs quickly.

Verified step by step guidance

1. Step 1: An exergonic reaction is a chemical reaction where the change in the Gibbs free energy is negative, indicating a spontaneous reaction. This means that the products of the reaction have lower Gibbs free energy than the reactants. So, the statement 'The products have lower Gibbs free energy than the reactants.' is True.
2. Step 2: Even though exergonic reactions are spontaneous, they still require a certain amount of energy to get started. This is known as the activation energy. Therefore, the statement 'Activation energy is required for the reaction to proceed.' is True.
3. Step 3: The entropy, or disorder, of a system can increase or decrease during an exergonic reaction. It is not always the case that the products have lower entropy than the reactants. Therefore, the statement 'The products always have lower entropy than the reactants.' is False.
4. Step 4: The speed at which an exergonic reaction occurs is not determined by the change in Gibbs free energy, but by the activation energy. Some exergonic reactions can occur quickly, while others can take a long time. Therefore, the statement 'The reaction always occurs quickly.' is False.
5. Step 5: In summary, for an exergonic reaction, the products have lower Gibbs free energy than the reactants and activation energy is required for the reaction to proceed. However, the products do not always have lower entropy than the reactants and the reaction does not always occur quickly.

Key Concepts

Exergonic Reactions

Exergonic reactions are chemical processes that release energy, typically in the form of Gibbs free energy. In these reactions, the products have lower Gibbs free energy than the reactants, indicating that the reaction can occur spontaneously. This energy release is crucial for various biological processes, such as cellular respiration.

Gibbs Free Energy

Gibbs free energy (G) is a thermodynamic quantity that combines enthalpy and entropy to predict the spontaneity of a reaction. A negative change in Gibbs free energy (ΔG < 0) signifies that a reaction is exergonic and can occur without external energy input. Understanding Gibbs free energy helps in determining the favorability of biochemical reactions.

Activation Energy

Activation energy is the minimum energy required for a chemical reaction to occur. Even in exergonic reactions, activation energy is necessary to initiate the process, as it helps overcome the energy barrier for the reactants to transform into products. This concept is essential for understanding reaction kinetics and the role of enzymes in biological systems.