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Chapter 16: Problem 9

Define the terms "endergonic" and "exergonic."

Short Answer

Expert verified
Endergonic reactions absorb energy and are non-spontaneous, while exergonic reactions release energy and are spontaneous.

Step by step solution

01

Understand Endergonic Reactions

Endergonic reactions are chemical reactions that absorb energy from their surroundings. In these processes, the products have a higher free energy than the reactants, resulting in a positive change in Gibbs free energy (\( \Delta G > 0\) ). Since they require an input of energy to proceed, these reactions are non-spontaneous.
02

Understand Exergonic Reactions

Exergonic reactions, on the other hand, release energy to their surroundings. In these reactions, the products have lower free energy than the reactants, resulting in a negative change in Gibbs free energy (\( \Delta G < 0\) ). These reactions are spontaneous, occurring without the need for additional energy.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Endergonic Reactions
Endergonic reactions involve the absorption of energy from the surroundings, essential for the reaction to proceed. In these chemical processes, the final products possess more free energy than the initial reactants, leading to a positive change in Gibbs free energy represented as \( \Delta G > 0 \).
This increase in energy means that the reaction does not happen on its own. The system requires input energy, often in the form of heat, light, or another form of chemical energy transfer.
  • For instance, the synthesis of glucose through photosynthesis is an endergonic reaction. Here, plants absorb sunlight energy to convert water and carbon dioxide into glucose and oxygen.
  • The necessity for external energy input makes these processes non-spontaneous under standard conditions.
Understanding endergonic reactions is crucial for fields like biochemistry, where many cellular processes rely on such energy-absorbing reactions to function effectively.
Exergonic Reactions
Exergonic reactions are characterized by the release of energy to the environment. These reactions proceed with a decrease in free energy, leading to a negative \( \Delta G < 0 \).
This means that exergonic reactions are often spontaneous, occurring without the need for continuous external energy once the process initiates.
  • Classic examples include cellular respiration, where glucose is broken down to release energy used by the cells.
  • Exergonic reactions are important in biology and industry because they provide energy necessary for various processes.
The spontaneous nature of exergonic reactions makes them fundamental in natural and engineered systems, where they help drive processes efficiently by liberating free energy.
Spontaneity of Reactions
The spontaneity of a chemical reaction is closely tied to its Gibbs free energy change. A crucial point to understand is that spontaneity refers to the ability of a reaction to proceed on its own without external input.
  • An exergonic reaction, with \( \Delta G < 0 \), is spontaneous because it releases energy as it progresses.
  • Conversely, an endergonic reaction, with \( \Delta G > 0 \), is non-spontaneous under normal conditions, requiring an external energy source.
Spontaneous processes are driven by the "desire" of systems to reach a state of lower energy and greater stability, which explains why exergonic reactions are more naturally favored in isolated systems.
In practical terms, understanding spontaneity is vital in predicting and controlling chemical reactions, essential in fields like chemistry, engineering, and environmental science.

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Most popular questions from this chapter

State five useful qualitative rules for predicting entropy changes when chemical or physical changes occur.

What are the two ways that a final chemical state of a system can be more probable than its initial state?

For each pair of items, predict which has the higher entropy, and explain why. (a) Item 1, a sample of solid \(\mathrm{CO}_{2}\) at \(-78^{\circ} \mathrm{C}\), or item \(2, \mathrm{CO}_{2}\) vapor at \(0{ }^{\circ} \mathrm{C}\) (b) Item 1, solid sugar, or item 2 , the same sugar dissolved in a cup of tea (c) Item 1, a 100-mL sample of pure water and a \(100-\mathrm{mL}\) sample of pure alcohol, or item 2 , the same samples of water and alcohol after they had been poured together and stirred

For each process, tell whether the entropy change of the system is positive or negative. (a) Water boils. (b) A teaspoon of sugar dissolves in a cup of coffee. (The system consists of both sugar and coffee.) (c) Calcium carbonate precipitates out of water in a cave to form stalactites and stalagmites. (Consider only the calcium carbonate to be the system.)

Appendix J lists standard molar entropies \(S^{\circ},\) not standard entropies of formation \(\Delta_{\mathrm{f}} S^{\circ} .\) Why is this possible for entropy but not for internal energy, enthalpy, or Gibbs free energy?
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