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
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
Related questions
Question
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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8356db49-748d-4110-bae4-35e11d46b97f%2F9ade6630-c0e2-48f4-913a-0f4153511af4%2Fm3rf2v_processed.png&w=3840&q=75)
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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