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Given the following equations and ΔH values, determine the heat of reaction (kJ) at 298 K for the reaction: B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) BCl3(g)+ 3 H2O(l)→ H3BO3(g)+ 3 HCl(g) ΔH = -112.5 kJ B2H6(g)+ 6 H2O(l)→ 2 H3BO3(s)+ 6 H2(g) ΔH = -493.4 kJ ½ H2(g) + ½Cl2(g) → HCl(g) ΔH = -92.3 kJ

Given the following equations and ΔH values, determine the heat of reaction (kJ) at 298 K for the reaction: B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) BCl3(g)+ 3 H2O(l)→ H3BO3(g)+ 3 HCl(g) ΔH = -112.5 kJ B2H6(g)+ 6 H2O(l)→ 2 H3BO3(s)+ 6 H2(g) ΔH = -493.4 kJ ½ H2(g) + ½Cl2(g) → HCl(g) ΔH = -92.3 kJ

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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Given the following equations and ΔH values, determine the heat of reaction
(kJ) at 298 K for the reaction:
B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g)
BCl3(g)+ 3 H2O(l)→ H3BO3(g)+ 3 HCl(g) ΔH = -112.5 kJ
B2H6(g)+ 6 H2O(l)→ 2 H3BO3(s)+ 6 H2(g) ΔH = -493.4 kJ
½ H2(g) + ½Cl2(g) → HCl(g) ΔH = -92.3 kJ

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