Explain why the equivalent weight of H2SO4 is half the molar mass of this substance. How many hydrogen ions does each H2SO4 molecule produce when reacting with an excess of OH ions?
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12.112.2 Spontaneous reactions simply need to be started with some added energy but then continue to react with no outside help until a reactant runs out. Such reactions may occur at any speed and may be exothermic or endothermic. While most spontaneous reactions are exothermic, certain endothermic reactions result in products which allow their particles to move more freely than in their reactant form, and therefore continue reacting to products naturally (spontaneous). This increased movement relates to entropy, which is how evenly distributed energy is in a system. According to the second law of thermodynamics, entropy in a closed system always increases, meaning energy becomes more diffused, through any s
Textbook: Introductory Chemistry: A Foundation
Author: Steven S. Zumdahl, Donald J. DeCoste
Introductory Chemistry: A Foundation was written by and is associated to the ISBN: 9781439049402. This textbook survival guide was created for the textbook: Introductory Chemistry: A Foundation, edition: 7. The full step-by-step solution to problem: 77 from chapter: 15 was answered by , our top Chemistry solution expert on 03/14/18, 08:03PM. This full solution covers the following key subjects: . This expansive textbook survival guide covers 21 chapters, and 2203 solutions. The answer to “Explain why the equivalent weight of H2SO4 is half the molar mass of this substance. How many hydrogen ions does each H2SO4 molecule produce when reacting with an excess of OH ions?” is broken down into a number of easy to follow steps, and 32 words. Since the solution to 77 from 15 chapter was answered, more than 233 students have viewed the full step-by-step answer.