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Liquid hydrogen peroxide is an oxidizing agent in rocket fuel mixtures because it decomposes to form oxygen, which is then used in the combustion of the rocket fuel. The reaction is: 2 H2O2 (1) → 2 H2O(1) + O2(8) AH = -196.1 K/mol If a 33.72 g sample of hydrogen peroxide is placed in a bomb calorimeter containing 372.9 g of water at 24.6 °C and allowed to react, what will be the final temperature of the water? Assume that the calorimeter absorbs a negligible amount of heat.

Liquid hydrogen peroxide is an oxidizing agent in rocket fuel mixtures because it decomposes to form oxygen, which is then used in the combustion of the rocket fuel. The reaction is: 2 H2O2 (1) → 2 H2O(1) + O2(8) AH = -196.1 K/mol If a 33.72 g sample of hydrogen peroxide is placed in a bomb calorimeter containing 372.9 g of water at 24.6 °C and allowed to react, what will be the final temperature of the water? Assume that the calorimeter absorbs a negligible amount of heat.

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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Liquid hydrogen peroxide is an oxidizing agent in rocket fuel mixtures because it decomposes to form oxygen, which is then used in the combustion of the rocket fuel. The reaction is: 2 H202 (1) → 2 H2O() + O2(8) AH = -196.1 K/mol If a 33.72 g sample of hydrogen peroxide is placed in a bomb calorimeter containing 372.9 g of water at 24.6 °C and allowed to react, what will be the final temperature of the water? Assume that the calorimeter absorbs a negligible amount of heat. °C
Transcribed Image Text:Liquid hydrogen peroxide is an oxidizing agent in rocket fuel mixtures because it decomposes to form oxygen, which is then used in the combustion of the rocket fuel. The reaction is: 2 H202 (1) → 2 H2O() + O2(8) AH = -196.1 K/mol If a 33.72 g sample of hydrogen peroxide is placed in a bomb calorimeter containing 372.9 g of water at 24.6 °C and allowed to react, what will be the final temperature of the water? Assume that the calorimeter absorbs a negligible amount of heat. °C
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