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Show complete solution. Round everything to four decimal places and box all final answers. The molar heat of formation of NH4NO3 (s) is -367.54 KJ and those of N20 (g) and H20 (1) are 81.46 and -285.8 KJ respectively at 25°C and 1 atmospheric pressure. Calculate

Show complete solution. Round everything to four decimal places and box all final answers. The molar heat of formation of NH4NO3 (s) is -367.54 KJ and those of N20 (g) and H20 (1) are 81.46 and -285.8 KJ respectively at 25°C and 1 atmospheric pressure. Calculate

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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Show complete solution. Round everything to four decimal places and box all final answers. The molar heat of formation of NH4N03 (s) is -367.54 KJ and those of N20 (g) and H20 (1) are 81.46 and -285.8 KJ respectively at 25°C and 1 atmospheric pressure. Calculate delta H and delta U of reaction. NH4NO3(s) → N20(g) + H20(I)
Transcribed Image Text:Show complete solution. Round everything to four decimal places and box all final answers. The molar heat of formation of NH4N03 (s) is -367.54 KJ and those of N20 (g) and H20 (1) are 81.46 and -285.8 KJ respectively at 25°C and 1 atmospheric pressure. Calculate delta H and delta U of reaction. NH4NO3(s) → N20(g) + H20(I)
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