Final answer:
The standard free energy change of 3.67 cal/mol indicates that the chemical reaction is not spontaneous under standard conditions. The reaction requires energy to occur.
Step-by-step explanation:
The standard free energy change of a chemical reaction, denoted as ΔG°, is calculated to be 3.67 cal/mol. The standard free-energy change (ΔG°) is the change in free energy when one substance or a set of substances in their standard states is converted to one or more other substances, also in their standard states.
The positive value of the standard free energy change (3.67 cal/mol) indicates that the reaction is not spontaneous under standard conditions. In order for the reaction to proceed spontaneously, the standard free energy change must be negative. Therefore, this reaction requires energy to occur.
It is important to note that the standard free energy change is calculated under standard conditions (pH 7.0, 25 degrees Celsius, and 1 atm pressure), and actual free energy values for reactions may differ in biological systems.