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a. Consider the endothermic reaction: 2 HgO (s) → 2 Hg (l) + O2 (g),  ΔH = 181.66 kJ/mol b. Consider the reaction: 2 C (graphite) + O2 (g) → 2 CO (g),  ΔH = –221 kJ/mol c. Consider the endothermic reaction: CdSO4 (s) → Cd2+ (aq) + SO42− (aq),    > 0 This reaction is nonspontaneous spontaneous at all temperatures spontaneous at low temperatures spontaneous at high temperatures

a. Consider the endothermic reaction: 2 HgO (s) → 2 Hg (l) + O2 (g),  ΔH = 181.66 kJ/mol b. Consider the reaction: 2 C (graphite) + O2 (g) → 2 CO (g),  ΔH = –221 kJ/mol c. Consider the endothermic reaction: CdSO4 (s) → Cd2+ (aq) + SO42− (aq),    > 0 This reaction is nonspontaneous spontaneous at all temperatures spontaneous at low temperatures spontaneous at high temperatures

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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a. Consider the endothermic reaction: 2 HgO (s) → 2 Hg (l) + O2 (g),  ΔH = 181.66 kJ/mol

b. Consider the reaction: 2 C (graphite) + O2 (g) → 2 CO (g),  ΔH = –221 kJ/mol

c. Consider the endothermic reaction: CdSO4 (s) → Cd2+ (aq) + SO42− (aq),    > 0

This reaction is

nonspontaneous

spontaneous at all temperatures

spontaneous at low temperatures

spontaneous at high temperatures

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