CHEM-ENG 333 Lecture 3: ChE_333_Lecture_3
28 views16 pages
18 Apr 2016
School
Department
Course
Professor
Get access
Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers
Class+
$8 USD/m
Billed $96 USD annually
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
30 Verified Answers
Related textbook solutions
Chemistry: Structure and Properties
2 Edition,
Tro
ISBN: 9780134293936
Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232
Related Documents
Related Questions
It is a hot summer day and Chris wants a glass of lemonade. There is none in the refrigerator, so a new batch is prepared from freshly squeezed lemons. When finished, there are 201grams of lemonade at 23.8°C. That is not a very refreshing temperature, so it must be cooled with ice. But Chris doesnât like ice in lemonade! Therefore, just enough ice is used to cool the lemonade to 10.5°C. Of course, the ice will melt and reach the same temperature. If the ice starts at -14.3°C, and if the specific heat of lemonade is the same as that of water, how many grams of ice does Chris use? Assume there is no heat transfer to or from the surroundings.
Data for water at 1 atm: |
Melting point = 0.0°C |
Specific heat liquid = 4.18 J/g·°C |
Specific heat solid = 2.06 J/g·°C |
Heat of fusion = 333 J/g |
__g