A sample of the sugar D-ribose (C5H10O5) of mass 0.727 g was placed in a constant volume calorimeter and then ignited in the presence of excess oxygen. The temperature rose by 0.910 K. In a separate experiment in the same calorimeter, the combustion of 0.825 g of benzoic acid, for which the internal energy of combustion is -3251 kJ mol-1, gave a temperature rise of 1.940 K. Calculate the internal energy of combustion of D-ribose and its enthalpy of formation. Combustion Reaction: 5 C (s) + 5 H2 (g) + 2/5 O2 (g) → C3H1,O5 (s) 5 C (s) + 5 O2 (g) → 5 CO2 (g) 5 H (g) + 2/5 О2 (g) - 5 СО2 (g) + 5 Н-0 (I) — CSH10O5 (s) + 5 Оz (g) AH°F298 = (5) (-39.351 x 107) AH°F298 = (5) (-28.584 x 10’) AH°r298 — 5 H-0 (1)
A sample of the sugar D-ribose (C5H10O5) of mass 0.727 g was placed in a constant volume calorimeter and then ignited in the presence of excess oxygen. The temperature rose by 0.910 K. In a separate experiment in the same calorimeter, the combustion of 0.825 g of benzoic acid, for which the internal energy of combustion is -3251 kJ mol-1, gave a temperature rise of 1.940 K. Calculate the internal energy of combustion of D-ribose and its enthalpy of formation. Combustion Reaction: 5 C (s) + 5 H2 (g) + 2/5 O2 (g) → C3H1,O5 (s) 5 C (s) + 5 O2 (g) → 5 CO2 (g) 5 H (g) + 2/5 О2 (g) - 5 СО2 (g) + 5 Н-0 (I) — CSH10O5 (s) + 5 Оz (g) AH°F298 = (5) (-39.351 x 107) AH°F298 = (5) (-28.584 x 10’) AH°r298 — 5 H-0 (1)
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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Transcribed Image Text:A sample of the sugar D-ribose (C5H10O5) of mass 0.727 g was placed in a constant volume
calorimeter and then ignited in the presence of excess oxygen. The temperature rose by 0.910 K.
In a separate experiment in the same calorimeter, the combustion of 0.825 g of benzoic acid, for
which the internal energy of combustion is -3251 kJ mol-1, gave a temperature rise of 1.940 K.
Calculate the internal energy of combustion of D-ribose and its enthalpy of formation.
Combustion Reaction: 5 C (s) + 5 H2 (g) + 2/5 O2 (g) → C3H19O5 (s)
5 С (5) + 5 02 (g) > 5 СO2 (g)
5 H2 (g) + 2/5 O2 (g) → 5 H2O (1)
5 СО2 (g) + 5 Н.O (1) — СsHi0Os (s) + 5 0г (g)
AH°F298 = (5) (-39.351 x 107)
AH°F298 = (5) (-28.584 x 107)
AH°F
F298 =
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