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?(a) Does the entropy of the surroundings increase for spontaneous processes? (b) In a particular spontaneous process the entropy of the syst

Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus ISBN: 9780134414232 1274

Solution for problem 19.26 Chapter 19

Chemistry: The Central Science | 14th Edition

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Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

Chemistry: The Central Science | 14th Edition

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Problem 19.26

(a) Does the entropy of the surroundings increase for spontaneous processes?

(b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of \(\Delta S_{\text {surr }}\)?

(c) During a certain reversible process, the surroundings undergo an entropy change, \(\Delta S_{\text {surr }}=-78 \mathrm{~J} / \mathrm{K}\). What is the entropy change of the system for this process?

Text Transcription:

\Delta S_surr

\Delta S_surr=-78 J/K

Step-by-Step Solution:

Step 1 of 5) Nuclear transmutations have been used to produce the elements with atomic number above 92, collectively known as the transuranium elements because they follow uranium in the periodic table. Elements 93 (neptunium, Np) and 94 (plutonium, Pu) were produced in 1940 by bombarding uranium-238 with neutrons: Elements with still larger atomic numbers are normally formed in small quantities in particle accelerators. Curium-242, for example, is formed when a plutonium-239 target is bombarded with accelerated alpha particles:New advances in the detection of the decay patterns of single atoms have led to recent additions to the periodic table. Between 1994 and 2010, elements 110 through 118 were discovered via the nuclear reactions that occur when nuclei of much lighter elements collide with high energy. For example, in 1996 a team of European scientists based in Germany synthesized element 112, copernicium, Cn, by bombarding a lead target continuously for three weeks with a beam of zinc atoms:

Step 2 of 2

Chapter 19, Problem 19.26 is Solved
Textbook: Chemistry: The Central Science
Edition: 14
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
ISBN: 9780134414232

This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 14. Since the solution to 19.26 from 19 chapter was answered, more than 214 students have viewed the full step-by-step answer. The answer to “?(a) Does the entropy of the surroundings increase for spontaneous processes? (b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of \(\Delta S_{\text {surr }}\)? (c) During a certain reversible process, the surroundings undergo an entropy change, \(\Delta S_{\text {surr }}=-78 \mathrm{~J} / \mathrm{K}\). What is the entropy change of the system for this process?Text Transcription:\Delta S_surr\Delta S_surr=-78 J/K” is broken down into a number of easy to follow steps, and 71 words. This full solution covers the following key subjects: . This expansive textbook survival guide covers 29 chapters, and 2820 solutions. The full step-by-step solution to problem: 19.26 from chapter: 19 was answered by , our top Chemistry solution expert on 10/03/18, 06:29PM. Chemistry: The Central Science was written by and is associated to the ISBN: 9780134414232.

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?(a) Does the entropy of the surroundings increase for spontaneous processes? (b) In a particular spontaneous process the entropy of the syst