If the Delta G of a reaction was -31.45kJoules you would know that: Multiple Choice the reaction is spontaneous. the products have more free energy than the reactants. the reaction requires an energy input of 3145 kJoules to proceed. the reaction most likely leads to development of a more ordered system.

**1. **Understanding :** The symbol represents the change in Gibbs free energy for a process at constant pressure and temperature. Gibbs free energy is a thermodynamic potential that measures the maximum reversible work that may be performed by a thermodynamic system at a constant temperature and pressure.2. **Interpreting the Sign of :** - A **negative** indicates that the process can occur spontaneously, meaning it does not require energy input to proceed. This is because the system is releasing free energy. - A **positive** would suggest that the process is non-spontaneous and requires energy input to proceed.3. **Evaluating the Choices:** - **Spontaneous Reaction:** The given kJoules directly implies that the reaction is spontaneous. - **Products vs. Reactants Energy:** If is negative, it means that the free energy of the reactants is higher than that of the products, not the other way around. Therefore, the statement that "the products have more free energy than the reactants" is incorrect in this context. - **Energy Input Required:** Since is negative, the reaction releases energy rather than requiring an external energy input of 31.45 kJoules to proceed. Hence, this choice is incorrect. - **Orderliness of the System:** A negative typically indicates that the reaction leads to a decrease in free energy, which can be associated with increased stability but does not directly correlate with the development of a more ordered system. The spontaneity of a reaction (indicated by a negative ) can lead to either more or less order depending on the nature of the reactants and products.**