
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
![The first step in the production of high purity silicon for
semiconductors is represented by this equation: SiO2(s) + 2C(s) -
Looking for 33 [right] given
answers below
Si(s) + 2CO(g) A H° = 689.9 kJ
Using the value of A Srxn you calculated from question 10 and/or
the value of A G° for the reaction at 25 °C you found in question 11,
find the minimum temperature in °C at which this reaction is
spontaneous. Assume that A H° and A Sº do not vary with
temperature.
-271.2 oC
1.912 oC
1639 oC
1912 oC
1614 oC
delta S-rxn
delta G*
The first step in the production of high purity silicon for
semiconductors is represented by this equation: SiO2(s) + 2C(s) →
Si(s) + 2CO(g) A Hº = 689.9 kJ
The first step in the production of high purity silicon for
semiconductors is represented by this equation: SiO2(s) + 2C(s) –→
Si(s) + 2CO(g) A Hº = 689.9 kJ
Using the value of A Srxnº you calculated from question 10,
determine A G° for the reaction at 25 °C.
Find A Srxnº for the production of pure silicon, given the following
data: S° for C = 5.7 J/mol*K, for CO = 197.6 J/mol*K, for Si = 18.8
J/mol*K and for SiO2 = 41.8 J/mol*K.
329.1 kJ/mol
582.3 kJ/mol
O O J/mol*K
O kJ/mol
60.8 J/mol*K
106.8 kJ/mol
O 2314 J/mol*K
O -106.8 kJ/mol
-360.8 J/mol*K
168.9 J/mol*K](https://content.bartleby.com/qna-images/question/71da7845-386a-4918-a86a-c17dc7624319/441707ee-9565-4080-93a4-82048dba639a/50bena_thumbnail.png)
Transcribed Image Text:The first step in the production of high purity silicon for
semiconductors is represented by this equation: SiO2(s) + 2C(s) -
Looking for 33 [right] given
answers below
Si(s) + 2CO(g) A H° = 689.9 kJ
Using the value of A Srxn you calculated from question 10 and/or
the value of A G° for the reaction at 25 °C you found in question 11,
find the minimum temperature in °C at which this reaction is
spontaneous. Assume that A H° and A Sº do not vary with
temperature.
-271.2 oC
1.912 oC
1639 oC
1912 oC
1614 oC
delta S-rxn
delta G*
The first step in the production of high purity silicon for
semiconductors is represented by this equation: SiO2(s) + 2C(s) →
Si(s) + 2CO(g) A Hº = 689.9 kJ
The first step in the production of high purity silicon for
semiconductors is represented by this equation: SiO2(s) + 2C(s) –→
Si(s) + 2CO(g) A Hº = 689.9 kJ
Using the value of A Srxnº you calculated from question 10,
determine A G° for the reaction at 25 °C.
Find A Srxnº for the production of pure silicon, given the following
data: S° for C = 5.7 J/mol*K, for CO = 197.6 J/mol*K, for Si = 18.8
J/mol*K and for SiO2 = 41.8 J/mol*K.
329.1 kJ/mol
582.3 kJ/mol
O O J/mol*K
O kJ/mol
60.8 J/mol*K
106.8 kJ/mol
O 2314 J/mol*K
O -106.8 kJ/mol
-360.8 J/mol*K
168.9 J/mol*K
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 2 steps

Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Given the data in the table in the figure at 1 atm and 25.0 °C, calculate the standard heat of reaction, ∆H°₂₅, for the reaction Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s) A) 216.8 kJ are evolved per mole B) 88.0 kJ are evolved per mole C) 88.0 kJ are absorbed per mole D) 216.8 kJ are absorbed per molearrow_forwardWhich of the following can NOT be deduced from the value of ArGº for a reaction? Select one: the total energy that is absorbed or released by the system during reaction. the value of the equilibrium constant, K, for the reaction. the amount of work that can be obtained from or is required for a reaction or process under standard conditions. the direction (forwards or reverse) of the spontaneous overall reaction.arrow_forwardUse standard thermodynamic data to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 20.46 mm Hg.2NO(g) + O2(g)2NO2(g) G = ______kJ/molarrow_forward
- A mole of sodium met is added to water How much work is done on the atmosphere by the subsequent reaction if the temperature is 25 C°arrow_forward65arrow_forwardA piece of Al(s) at 91°C is placed in 69g of H2O at 27°C. The Aluminum cools and after equilibrium the final temperature of Aluminum and water is 35°C. What was the mass of the aluminum?Cs(H2O)= 4.184J/(g°C)Cs(Al)= 0.90J/(g.°C) garrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning

Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning

Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning

Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY