1/9/2023
Week 1 - Lecture 1
Course Overview & Review Material
Prof. Farmer
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Welcome to CHE112
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Some important netiquette reminders during lecture:
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If you have a question, please raise your hand.
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Be present and kind (we are all in this together and are all here to learn)
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Be supportive of each other and the teaching team – we all want you to succeed!
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Ask questions (there are no silly questions) and have fun!
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Engage in discussion with your peers. However, when someone is talking please be
respectful and give them your attention
Lecture: Time & Date
Location
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Mon. 4-5pm
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MP202
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Tue. 5-6pm
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MP202
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Thu. 4-5pm
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MP202
NOTE: Tutorials begin next week and Quercus pages will be activated later this week.
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TUT0101 (Mon. 12-2pm) – ESB149
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TUT0104 (Fri. 10 am -12pm) – BA1200
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TUT0102 (Wed. 12-2pm) – HS108
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TUT0106 (Tue. 3-5 pm) – BA1230
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TUT0103 (Wed. 12-2pm) – BA2185
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Teaching Team
Course Instructor & Coordinator: Prof. Jennifer Farmer
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Department: Chemical Engineering and Applied Chemistry & ISTEP
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Office Hours: Friday 3-4pm (tentative). Will finalize during lecture 1. If you
cannot make these office hours, please email me to set up an
appointment. Office: WB216B (inside UG Office)
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Email: jennifer.farmer@utoronto.ca
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Research Interests:
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Chemical and engineering education (focus in undergraduate
laboratory instructions and active learning pedagogy)
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Biofuels (studying the effects of solid-supported catalysts in the
production of biodiesel)
Hobbies/Passions: cycling, cooking, gardening, taking care of my reptiles,
drinking coffee and of course teaching ☺
Teaching Assistants:
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Sepehr Hoomani Rad
(sepehr.hoomanirad@mail.utoronto.ca)
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Runlin Yuan
(runlin.yuan@mail.utoronto.ca)
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Saif Rjaibi
(saif.rjaibi@mail.utoronto.ca)
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Chengqian Wu
(chengqian.wu@mail.utoronto.ca)
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Arianna Skirzynska
(arianna.skirzynska@mail.utoronto.ca)
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Course Overview
Course Description:
• CHE112 presents the basics of physical chemistry including a range of physical
phenomena that are fundamental to the engineering discipline.
• Concepts are important when designing processes that utilize gases, liquids and
solids, and involve chemical and physical changes.
• In this course, you will learn how to use theoretical and mathematical equations to
understand chemical properties and structure of matter, and their relation to the
interaction of matter with energy.
• Topics include:
• States of matter
• Chemical equilibrium
• Properties of gases
• Solutions (or mixtures)
• Chemical reactions
• Colligative properties
• Phase equilibrium
• Electrochemistry & corrosion (time permitting)
• The laws of thermodynamics (calculations involving internal energy, enthalpy, free energy and
entropy)
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Course Overview
Course Goals:
• The overall goals of this course is to provide students with an:
• understanding of the concepts and basic principles of thermodynamics and
equilibrium processes
• appreciation for how theory and mathematical laws can be used to explain and to
predict experimental behaviour
• opportunity to apply critical thinking and analysis skills to offer solutions to realworld problems
• appreciation for the various applications of physical chemistry in chemical
engineering (e.g., industrial processes biological systems, etc.)
• Road to Success. You will meet the outcomes listed on the next slide through a
combination of the following activities in this course:
• Attend lectures and tutorials
• Complete assigned readings and watching videos, problem sets, self-quizzes and
assessments
• Participate in discussions and work with group members or classmates to complete
assignments
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Review Intended learning outcomes in Course Syllabus
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Course Syllabus
Textbook:
• Physical Chemistry for Engineering and Applied Chemistry by F. R. Foulkes
(ISBN: 978-1-4665-1846-9)
Available through U of T Engineering Library & Book Store.
Other Resources: You may find it useful to use other online sources to aid in your
learning process. Below are a few excellent free online resources.
• Open Stax Textbook: Chemistry 2e (good textbook with lots of addition problems and
solutions)
• Crash Course: Chemistry and Crash Course: Physics (great summary videos for
theoretical understanding)
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Course Outline
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Study Tips
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Before coming to lecture, complete assigned readings and review lecture slides (slides will be
posted before lecture on Quercus).
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Course Outline
▪
Study Tips
▪
Before coming to lecture, complete assigned readings and review lecture slides (slides will be
posted before lecture on Quercus).
▪
If you don’t have enough time review “Key Points” at end of chapter.
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Course Outline
▪
Study Tips
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Before coming to lecture, complete assigned readings and review lecture slides (slides will be
posted before lecture on Quercus). If you don’t have enough time review “Key Points” at end of
chapter.
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Take notes in class and try to record the main ideas If you cannot attend class, listen to
recordings and make notes.
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Attend lectures, participate in class discussions and attempt practice problems assigned in
class.
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After each lecture, review your notes and summarize the major ideas and concepts in
connection with the textbook.
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Attempted problem sets prior to attending tutorials. Problems will be related to lectures and
suggested readings. Problems will be selected from a variety of sources and answers will be
posted towards the end of the week (after all tutorial sections have met). These problems will
help identify areas of strength in your knowledge and areas to review.
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Complete self-quizzes. These will help you stay on top of topics and help you identify areas of
strength and weakness.
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Dedicate a certain amount of time per week for this course to avoid becoming overwhelmed
the night before a class quiz, midterm or final
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Reach out for help (to your TAs, classmates, Prof. Farmer)!
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Course Structure
Assessment Percent Details
Due Date
Participation
5%
Attendance will be taken in tutorial throughout the term and will be No Specific Date
Grading Scheme
used to compute this grade. Students must be active participants to
(assessed during
receive full marks – simply showing up is not enough.
each tutorial)
Self-Quiz
5%
Quizzes will be online and made available through Quercus. Quizzes No Specific Date
will be released with each module. There will be 6 in total, but only
(due dates will be
the top 5 will count towards the student's grade. The intent of these
posted on Quercus)
quizzes is to help you stay on track with course material and to have
you assess your own learning process at your own pace. Question are
designed to be straight forward and target specific concepts. Level of
difficulty will range from easy to medium.
Midterm
30%
March 7 is the tentative date (waiting for confirmation). If there are 2023-03-07
any changes you will be notified via a Quercus announcement.
Assignment
15%
Final Exam
45%
Working in groups you will research, design and execute your own No Specific Date
lab using readily accessible materials. The goal of this assignment is
Lectures: every Wed.
10-12
(EST) with your peers while applying course concepts
to have
you engage
to broader contexts. Completion of this assignment will give you a
Tutorials: every Thu
1-2pm
(EST)
deeper understanding of the course material and how it relates to
the engineering discipline or everyday life. Further details will be
posted on Quercus.
The final exam covers all course material presented during the term.
Final Exam Period
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Course Structure
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Course Structure
Tasks:
• Complete Module 0 - “How this Course Works”
• Complete Module 1 Readings
Quizzes:
• Self Assessment – Chemistry Review Quiz (not
graded, completion counts towards bonus mark)
complete by Jan. 13
• Information will be used to help teaching team
prepare materials for Tutorial 1
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Course Readings and Outline Summary
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Summarizes topics for each unit. Can use this schedule to keep track of readings
and read ahead!
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Subject to change depending on pace of class. Please check regularly for updates.
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Course Readings and Outline Summary
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Review of Fundamentals
Unit Conversion &
Stoichiometry
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Review Material
Sig. figs in a quantity indicate the number of known values (digits) in a measurement and number of
digits we use to report values has meaning.
Significant Figures Rules
• When reporting a results or performing a calculation, not only is it important to keep track of our units but
we also need to keep track of the number of significant figures.
• Rule 1: All nonzero digits are significant (e.g., 2.345 m _____ ; 9.86g _______ )
• Rule 2: Final zeros to the right of the decimal place are significant (e.g., 2.0km _____ ; 6.300cm _____ )
• Rule 3: Zeros found between two significant figures are significant (e.g., 23.0005g _____ )
• Rule 4: Zeros as placeholders are not significant (e.g., 0.0038g _______ )
Scientific Notation
• For simplicity, to represent large or small numbers 0.00000001 g, use scientific notation:
• 602 213 670 000 000 000 000 particles → 6.022 1367 x 1023 particles
• 0.000000000000001 g → 1 x 10-15 g
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Review Material
Sig. figs in a quantity indicate the number of known values (digits) in a measurement and number of
digits we use to report values has meaning.
Significant Figures Rules
• When reporting a results or performing a calculation, not only is it important to keep track of our units but
we also need to keep track of the number of significant figures.
• Rule 1: All nonzero digits are significant (e.g., 2.345 m _____ ; 9.86g _______ )
• Rule 2: Final zeros to the right of the decimal place are significant (e.g., 2.0km _____ ; 6.300cm _____ )
• Rule 3: Zeros found between two significant figures are significant (e.g., 23.0005g _____ )
• Rule 4: Zeros as placeholders are not significant (e.g., 0.0038g _______ )
Scientific Notation
• For simplicity, to represent large or small numbers 0.00000001 g, use scientific notation:
• 602 213 670 000 000 000 000 particles → 6.022 1367 x 1023 particles
• 0.000000000000001 g → 1 x 10-15 g
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Review Material
• Significant Figures Calculations:
• Multiplication and Division: Round final answer to the same number of sig figs (SF) as
factor with fewest SF.
Example: 3.06cm x 12.1 cm x 110 cm = 4072.86 or 4.1 x 103 cm3 (2 SF - round to least accura
te. Round up since 7 is greater than 5 as it would be incorrect to write 4.0 x 103 cm3).
• Addition and Subtractions: Round to fewest decimal places past the decimal.
Example: 3.05cm + 12.1 cm = 15.15 or 15.16 or 15.2 cm (3 SF – round to least accurate
which is 1 place past decimal. Since a 6 follows the 1 after the decimal place, we round up).
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Review Material
• Significant Figures Calculations:
• Multiplication and Division: Round final answer to the same number of sig figs (SF) as factor
with fewest SF.
Example: 3.06cm x 12.1 cm x 110 cm = 4072.86 or 4.1 x 103 cm3 (2 SF - round to least accurate. Round up
since 7 is greater than 5 as it would be incorrect to write 4.0 x 103 cm3).
• Addition and Subtractions: Round to fewest decimal places past the decimal.
Example: 3.05cm + 12.1 cm = 15.15 or 15.2 cm (3 SF – round to least accurate which is 1 place past
decimal. Since a 6 follows the 1 after the decimal place, we round up).
If the last digit discarded is 5 or greater, increase the last remaining digit by one; if
less than 5, leave the remaining digit unchanged.
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Review Material
Rounding Off Numbers
• Generally, rounding off of numbers calculated from observed quantities should be performed
after all calculations are complete, taking into account the cumulative uncertainty of the final
result.
• Don’t round at intermediate steps (unless otherwise stated) in a calculation since
information may be lost to “rounding errors”. Final answers are generally rounded.
Example: [(6.626 x 10-34)(7.3 x 1014)] – 4.6 x 10-19 = 2.4 x 10-20
INCORRECT: [(6.626 x 10-34)(7.3 x 1014)] = 4.83698 x 10-19 ≅ 4.8 x 10-19 – 4.6 x 10-19 = 2.0 x 10-20
Since successive rounding can compound inaccuracies, intermediate rounding can be done but
with care (general rule is to keep at least one more digit than required).
CORRECT: [(6.626 x 10-34)(7.3 x 1014)] = 4.83698 x 10-19 ≅ 4.84 x 10-19 – 4.6 x 10-19 = 2.4 x 10-20
If the last digit discarded is 5 or greater, increase the last remaining digit by one; if
less than 5, leave the remaining digit unchanged.
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Review Material
Rounding Off Numbers
• Generally, rounding off of numbers calculated from observed quantities should be performed
after all calculations are complete, taking into account the cumulative uncertainty of the final
result.
• Don’t round at intermediate steps (unless otherwise stated) in a calculation since
information may be lost to “rounding errors”. Final answers are generally rounded.
Example: [(6.626 x 10-34)(7.3 x 1014)] – 4.6 x 10-19 = 2.4 x 10-20
INCORRECT: [(6.626 x 10-34)(7.3 x 1014)] = 4.83698 x 10-19 ≅ 4.8 x 10-19 – 4.6 x 10-19 = 2.0 x 10-20
Since successive rounding can compound inaccuracies, intermediate rounding can be done but
with care (general rule is to keep at least one more digit than required).
CORRECT: [(6.626 x 10-34)(7.3 x 1014)] = 4.83698 x 10-19 ≅ 4.84 x 10-19 – 4.6 x 10-19 = 2.4 x 10-20
If the last digit discarded is 5 or greater, increase the last remaining digit by one; if
less than 5, leave the remaining digit unchanged.
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Review Material
• Dimensional Analysis (Unit Conversions):
• As Engineers, you will see a variety of numbers in a variety of units. In Canada we use the
SI system but in places like the USA they still use the British system. Given that we trade
with the USA, you need to be comfortable understanding the different systems and how to
convert units between the two.
• Engineers must be skilled in unit analysis. Knowing the unit(s) you are given and the units
you want to end up with is really the key to unit conversion.
Knowing 1L = $0.3/L
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Review Material
• Dimensional Analysis (Unit Conversions):
• As Engineers, you will see a variety of numbers in a variety of units. In Canada we use the
SI system but in places like the USA they still use the British system. Given that we trade
with the USA, you need to be comfortable understanding the different systems and how to
convert units between the two.
• Engineers must be skilled in unit analysis. Knowing the unit(s) you are given and the units
you want to end up with is really the key to unit conversion.
Example: Temperature
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Celsius scale (θ): 0.00 oC (typically used in Canada)
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Kelvin scale (T): T = θ + 273.15 (unit of absolute temperature)
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Fahrenheit scale (oF): oF = 9/5 θ + 32 (typically used in USA)
Homework: If the temperature of the human body is 98.6 oF, what is the vale in oC and K?
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Review Material
• Dimensional Analysis (Unit Conversions):
• As Engineers, you will see a variety of numbers in a variety of units. In Canada we use the
SI system but in places like the USA they still use the British system. Given that we trade
with the USA, you need to be comfortable understanding the different systems and how to
convert units between the two.
• Engineers must be skilled in unit analysis. Knowing the unit(s) you are given and the units
you want to end up with is really the key to unit conversion.
Example: Temperature
•
Celsius scale (θ): 0.00 oC (typically used in Canada)
•
Kelvin scale (T): T = θ + 273.15 (unit of absolute temperature)
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Fahrenheit scale (oF): oF = 9/5 θ + 32 (typically used in USA)
Homework: If the temperature of the human body is 98.6 oF, what is the vale in oC and K?
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Review Material
• Dimensional Analysis (Unit Conversions):
Example: Hand sanitizer is one way to protect yourself against COVID-19. A local grocery store
goes through 25 gallon of hand sanitizer a day to provide protection to its workers and
customers. What volume (in L) is required to supply the store for 1 month? Calculate using
both systems.
Imperial: 1 gallon (gal) = 4 quarts (qt); 1L = 0.879877 qt
US Liquids: 1 gallon (gal) = 4 quarts (qt); 1L = 1.0567 qt
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Review Material
• Dimensional Analysis (Unit Conversions):
Example: Hand sanitizer is one way to protect yourself against COVID-19. A local grocery store
goes through 25 gallon of hand sanitizer a day to provide protection to its workers and
customers. What volume (in L) is required to supply the store for 1 month? Calculate using
both system.
Imperial: 1 gallon (gal) = 4 quarts (qt); 1L = 0.879877 qt
US Liquids: 1 gallon (gal) = 4 quarts (qt); 1L = 1.0567 qt
Approach: When problem solving it’s important to clearly outline your approach so the reader
better understands your solution and how you arrive at your final value.
1. Understand the Question (what are you being asked?). Need to determine volume (units =
liters) for 1 month supply.
2. Assumptions. How many days are in 1 month? We will assume 30 days here.
3. Acknowledge conversion factors used. What system are we using? There is a difference
between Imperial gallon and U.S. liquid gallon.
Imperial system Answer: 3.4 x 103 L/month
US Liquid System Answer: 2.8 x 103 L/month
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Review Material - CORRECT
• Dimensional Analysis (Unit Conversions):
Example: Hand sanitizer is one way to protect yourself against COVID-19. A local grocery store
goes through 25 gallon of hand sanitizer a day to provide protection to it’s workers and
customers. What volume (in L) is required to supply the store for 1 month?
1 gallon (gal) = 4 quarts (qt); 1L = 0.879877 qt
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Review Material - CORRECT
• Dimensional Analysis (Unit Conversions):
Example: Hand sanitizer is one way to protect yourself against COVID-19. A local grocery store
goes through 25 gallon of hand sanitizer a day to provide protection to it’s workers and
customers. What volume (in L) is required to supply the store for 1 month?
1 gallon (gal) = 4 quarts (qt); 1L = 1.0567 qt
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Review Material
• Dimensional Analysis (Unit Conversions):
Example: Hand sanitizer is one way to protect yourself against COVID-19. A local grocery store
goes through 25 gallon of hand sanitizer a day to provide protection to its workers and
customers. What volume (in L) is required to supply the store for 1 month?
Homework: What if you were given the following conversion units?
1 gallon = 0.16 ft3; 1 ft3 = 28.31685 L (this is for imperial system)
Try the calculation and see if you can arrive at 3.4 x 103 L/month.
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Review Material
• Dimensional Analysis (Unit Conversions):
Example: Hand sanitizer is one way to protect yourself against COVID-19. A local grocery store
goes through 25 gallon of hand sanitizer a day to provide protection to its workers and
customers. What volume (in L) is required to supply the store for 1 month?
Homework: What if you were given the following conversion units?
1 gallon = 0.16 ft3; 1 ft3 = 28.31685 L (this is for imperial system)
Try the calculation and see if you can arrive at 3.4 x 103 L/month.
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Reminders
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Complete Chemistry Review Quiz by Jan. 13. Results will be used to help teaching
team put together resources for Tutorial 1.
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Sign-up for Piazza (see home page for link)
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Module 2 will be released by Friday, Jan. 13.
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Tutorials begin next week. Problem set #1 will be released by Wed. Jan. 11 and
taken up during next week’s tutorial. See road map for content.
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Review the course syllabus. If you have any concerns or question please do not
hesitate to contact Prof. Farmer
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Lecture content for remainder of Week 1
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Tuesday: Stoichiometry
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Thursday: States of Matter and Pressure and Temperature See you on Tuesday. We will start with a
quick review of some fundamental chemistry knowledge learned in high school. Review Module 1
content and Ch. 1 & Ch. 2 of Foulkes textbook.
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