Multiple Choice
An exergonic reaction __________ free energy, and an endergonic reaction __________ free energy.
1. Introduction to Biochemistry
Gibbs Free Energy
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Which of the following statements about endergonic reactions is true?
A
Endergonic reactions release free energy to the surroundings.
B
Endergonic reactions occur spontaneously under standard conditions.
C
Endergonic reactions always involve a decrease in entropy (\( \Delta S < 0 \)).
D
Endergonic reactions have a positive value of \( \Delta G \).
Verified step by step guidance1
Understand the concept of endergonic reactions: These are reactions that require an input of energy to proceed. They are non-spontaneous under standard conditions and are characterized by a positive Gibbs free energy change (
).
Recall the definition of Gibbs free energy (
): It represents the energy available to do work in a system. A positive
indicates that the reaction requires energy input.
Analyze the incorrect statements: Endergonic reactions do not release free energy to the surroundings; instead, they absorb energy. They are not spontaneous under standard conditions, and while entropy (
) can decrease, it is not a defining feature of endergonic reactions.
Focus on the correct statement: Endergonic reactions are defined by a positive Gibbs free energy change (
), which indicates that energy must be supplied for the reaction to proceed.
Summarize the reasoning: The defining characteristic of endergonic reactions is their positive Gibbs free energy change (
), which distinguishes them from exergonic reactions that release energy (
).
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