- The Gibbs free energy change \(\Delta G = -1.6\) is less than zero, indicating that the reaction is exergonic.
- Exergonic reactions occur spontaneously and release free energy.
- This released energy can be utilized to perform work.
- The correct classification is: \(\boxed{\text{exergonic, and work can be done with energy released from the reaction}}\).
Explanation
- Analysis of Gibbs Free Energy Change
In thermodynamics, the Gibbs free energy change, denoted as \(\Delta G\), determines the spontaneity of a chemical reaction under constant pressure and temperature. A reaction is classified based on the sign of \(\Delta G\). If \(\Delta G < 0\), the reaction is exergonic, meaning it occurs spontaneously and releases free energy into the surroundings. If \(\Delta G > 0\), the reaction is endergonic, meaning it is non-spontaneous and requires an input of energy to proceed. Given the value \(\Delta G = -1.6\), we observe that \(-1.6 < 0\).
- Classification of the Reaction and Work Capacity
Since the calculated \(\Delta G\) is less than zero (\(\Delta G = -1.6 < 0\)), we classify this reaction as exergonic. By definition, an exergonic reaction is a process that releases energy. This released free energy can be harnessed to perform cellular or chemical work. In contrast, an endergonic reaction requires an input of energy, effectively meaning work must be done on the system for the reaction to occur.
- Final Conclusion and Selection
Based on the classification as exergonic and the capacity for spontaneous energy release, the statement that correctly describes the reaction is: 'exergonic, and work can be done with energy released from the reaction'. Other options involving endergonic reactions or the need for input energy are incorrect because they contradict the thermodynamic properties of a system with \(\Delta G < 0\). Thus, the correct choice is the second one.
Examples
In biological systems, the hydrolysis of ATP is a classic example of an exergonic reaction where \(\Delta G\) is negative. This release of free energy is essential for powering various biological processes, such as muscle contraction, active transport of molecules across cell membranes, and the synthesis of complex macromolecules. Without the capacity of exergonic reactions to perform this work, life as we know it could not maintain its structure or function.