A reaction with a positive ΔG is:
Please choose the correct answer from the following choices,

Question

BlackTom AI · Accepted Answer

First, let's lay out the question and the available choices in plain terms: a reaction with a positive ΔG is being described, and we must pick which statement best fits that scenario.
Option 1: 'an exergonic reaction.' An exergonic reaction has a negative ΔG, meaning it releases free energy. Since our condition is a positive ΔG, this option is incorrect because it describes the opposite thermodynamic sign.
Option 2: 'dependent upon an input of free energy in order to occur.' A positive ΔG indicates that the reaction is non-spontaneous under standard conditions and requires an input of free energy to proceed. This aligns directly with the definition of positive ΔG, making this a correct description.
Option 3: 'at equilibrium.' At equilibrium, ΔG equals zero; there is no net drive in either direction. A positive ΔG would imply the reaction is not at equilibrium and would require energy input to reach proceeding, so this option is incorrect.
Option 4: 'always dependent upon energy input from ATP hydrolysis.' While many biologically relevant endergonic reactions are powered by ATP hydrolysis, not all reactions with positive ΔG must be driven by ATP hydrolysis specifically. Other energy sources or coupled processes can provide the required free energy. Thus this is not universally correct and can be misleading.
Option 5: 'never a useful biochemical reaction.' This is false because endergonic (positive ΔG) steps are essential in biology, often coupled to exergonic processes to drive biosynthesis and other cellular work. Declaring them never useful is incorrect.
In summary, the statement that best matches a reaction with a positive ΔG is that it is dependent upon an input of free energy in order to occur, since positive ΔG denotes non-spontaneity requiring energy input to proceed.

A reaction with a positive ΔG is: Please choose the correct answer from the following choices,

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