The most common form of elemental sulfur is Sg, in which eight sulfur atoms linked in a ring of single bonds. At high temperature, in the gas phase, Sg can break apart to give S₂, the sulfur analog of molecular oxygen: Sg(g) 4S₂(g) AH = +239 kJ at T = 800 K

The most common form of elemental sulfur is Sg, in which eight sulfur atoms linked in a ring of single bonds. At high temperature, in the gas phase, Sg can break apart to give S₂, the sulfur analog of molecular oxygen: Sg(g) 4S₂(g) AH = +239 kJ at T = 800 K

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

calculate the S=S double-bond energy (in kJ/mol) in S₂(g).

The most common form of elemental sulfur is Sg, in which eight sulfur atoms linked in a ring of single bonds. At high temperature, in the
gas phase, Sg can break apart to give S₂, the sulfur analog of molecular oxygen:
Sa(g) 45₂(g) AH = +239 kJ at T = 800 K

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