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Equations: AH =E (n · AHproducts) – E (n · AHreac tan ts) AS = E (n · ASproducts) – E (n · AS.rcac tan to) AG = E (n · AGproducts) – E (n · AGreac tan to) AG = AH - TAS Hydrogen peroxide, H2O2, decomposes into water and oxygen gas with an enthalpy (AH) change of -37.77 kJ and an entropy (AS) change of -130.92 JIK. Will this reaction be spontaneous if the H2O2 is kept in a sub-zero refrigerator at -25 °C?

Equations: AH =E (n · AHproducts) – E (n · AHreac tan ts) AS = E (n · ASproducts) – E (n · AS.rcac tan to) AG = E (n · AGproducts) – E (n · AGreac tan to) AG = AH - TAS Hydrogen peroxide, H2O2, decomposes into water and oxygen gas with an enthalpy (AH) change of -37.77 kJ and an entropy (AS) change of -130.92 JIK. Will this reaction be spontaneous if the H2O2 is kept in a sub-zero refrigerator at -25 °C?

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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answer question nine

### Math Short Answer #### Question 09 (6/10) **Equations:** - \(\Delta H = \sum (n \cdot \Delta H_{\text{products}}) - \sum (n \cdot \Delta H_{\text{reactants}})\) - \(\Delta S = \sum (n \cdot \Delta S_{\text{products}}) - \sum (n \cdot \Delta S_{\text{reactants}})\) - \(\Delta G = \sum (n \cdot \Delta G_{\text{products}}) - \sum (n \cdot \Delta G_{\text{reactants}})\) - \(\Delta G = \Delta H - T \Delta S\) Hydrogen peroxide, \( \text{H}_2\text{O}_2 \), decomposes into water and oxygen gas with an enthalpy (\(\Delta H\)) change of -37.77 kJ and an entropy (\(\Delta S\)) change of -130.92 J/K. Will this reaction be spontaneous if the \( \text{H}_2\text{O}_2 \) is kept in a sub-zero refrigerator at -25 °C? **Note from instructor (Abbey Rickelmann):** - "You needed to remember to multiply \(\Delta H\) by 1000." --- This section contains a short-answer question from a chemistry context, asking students to determine the spontaneity of a reaction involving hydrogen peroxide decomposition. The given equations and constants are crucial for understanding and solving the problem.
Transcribed Image Text:### Math Short Answer #### Question 09 (6/10) **Equations:** - \(\Delta H = \sum (n \cdot \Delta H_{\text{products}}) - \sum (n \cdot \Delta H_{\text{reactants}})\) - \(\Delta S = \sum (n \cdot \Delta S_{\text{products}}) - \sum (n \cdot \Delta S_{\text{reactants}})\) - \(\Delta G = \sum (n \cdot \Delta G_{\text{products}}) - \sum (n \cdot \Delta G_{\text{reactants}})\) - \(\Delta G = \Delta H - T \Delta S\) Hydrogen peroxide, \( \text{H}_2\text{O}_2 \), decomposes into water and oxygen gas with an enthalpy (\(\Delta H\)) change of -37.77 kJ and an entropy (\(\Delta S\)) change of -130.92 J/K. Will this reaction be spontaneous if the \( \text{H}_2\text{O}_2 \) is kept in a sub-zero refrigerator at -25 °C? **Note from instructor (Abbey Rickelmann):** - "You needed to remember to multiply \(\Delta H\) by 1000." --- This section contains a short-answer question from a chemistry context, asking students to determine the spontaneity of a reaction involving hydrogen peroxide decomposition. The given equations and constants are crucial for understanding and solving the problem.
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