/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 60 Are endothermic reactions never ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 12: Problem 60

Are endothermic reactions never spontaneous at low temperature? Explain your answer.

Short Answer

Expert verified
Answer: It is incorrect to say that endothermic reactions are never spontaneous at low temperatures. The spontaneity of a reaction depends on the Gibbs free energy (螖G), which is determined by the change in enthalpy (螖H), temperature (T), and change in entropy (螖S). In some cases, with a sufficiently large positive 螖S value, an endothermic reaction can still occur spontaneously at low temperatures.

Step by step solution

01

Understanding Gibbs Free Energy

Gibbs free energy (G) is an essential concept for determining whether a reaction is spontaneous or not. It is represented as: 螖G = 螖H - T螖S Where, 螖G is the change in Gibbs free energy, 螖H is the change in enthalpy, T is the temperature in Kelvin, and 螖S is the change in entropy. If 螖G < 0, the reaction is spontaneous. If 螖G > 0, the reaction is non-spontaneous. If 螖G = 0, the reaction is at equilibrium.
02

Understanding Endothermic Reactions

An endothermic reaction is a chemical reaction that absorbs heat from the surroundings. As a result, the change in enthalpy (螖H) for an endothermic reaction is positive.
03

Analyzing the Importance of Temperature in Spontaneity

The sign and magnitude of 螖G can highly depend on the temperature. If the temperature is high enough, it can make the reaction spontaneous even if the reaction is endothermic.
04

Analyzing Endothermic Reactions at Low Temperature

For an endothermic reaction with positive 螖H, if the temperature is low, the term T螖S can be smaller than 螖H. This means that the Gibbs free energy 螖G might stay positive, making the reaction non-spontaneous. However, this is not always the case. If the change in entropy (螖S) is large enough and positive, it can make the reaction spontaneous even at low temperatures, yielding a negative delta G value.
05

Conclusion

It is incorrect to say that endothermic reactions are never spontaneous at low temperatures. The spontaneity of a reaction depends on the Gibbs free energy (螖G), which is determined by the change in enthalpy (螖H), temperature (T), and change in entropy (螖S). In some cases, with a sufficiently large positive 螖S value, an endothermic reaction can still occur spontaneously at low temperatures.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Identify the following processes as spontaneous or nonspontaneous, and explain your choice. a. A photo voltaic cell in a portable device charges your cell phone. b. Dry icc (solid \(\mathrm{CO}_{2}\) ) sublimes at room temperature. c. A radio pharmaceutical imaging agent containing technetium emits gamma rays.

Methanogenic bacteria convert liquid acetic acid (CH \(_{3} \mathrm{COOH}\) ) into \(\mathrm{CO}_{2}(g)\) and \(\mathrm{CH}_{4}(g)\). a. Is this process endothermic or exothermic under standard conditions? b. Is the reaction spontaneous under standard conditions?

Diamond and the fullerenes are allotropes of carbon. On the basis of their different structures and properties, predict which has the higher standard molar entropy.

Which component in each of the following pairs has the greater entropy? a. 1 mole of \(\mathrm{S}_{2}(g)\) or 1 mole of \(\mathrm{S}_{8}(g)\) b. 1 mole of \(S_{2}(g)\) or 1 mole of \(S_{8}(s)\) c. 1 mole of \(\mathrm{O}_{2}(g)\) or 1 mole of \(\mathrm{O}_{3}(g)\)

Rank the compounds in each of the following groups in order of increasing standard molar entropy \(\left(S^{\circ}\right):\) a. \(\mathrm{CH}_{4}(g), \mathrm{CH}_{3} \mathrm{CH}_{3}(g),\) and \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}(g)\) b. \(\mathrm{CCl}_{4}(\ell), \mathrm{CHCl}_{3}(\ell),\) and \(\mathrm{CH}_{2} \mathrm{Cl}_{2}(\ell)\) c. \(\mathrm{CO}_{2}(\ell), \mathrm{CO}_{2}(g),\) and \(\mathrm{CS}_{2}(g)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.