CHEM 1050 Lecture 1: Introduction to Thermodynamics and Kinetics

Lecture Overview

  • Overview of topics to be covered in the course:

    • Definition of thermodynamics and kinetics.

    • Explanation of the SI unit system for energy.

    • Discussion on how to manage precision and uncertainty in measurements.

    • Introduction to a problem-solving strategy for CHEM 1050.

Course Administration

  • Instructor Information: Khashayar Ghandi, Email: kghandi@uoguelph.ca

  • Textbook Information:

    • Text: D. Ebbing & S. Gammon, General Chemistry.

    • Versions: 10th, 9th, or 8th edition can be used.

    • Key chapters: 6, 13, 18, 19; sections 9.1, 9.11 & 20.4.

  • Course Evaluation Schemes:

    • Scheme 1: Mastering Chemistry Homework contributes 10% to overall grade.

    • Scheme 2: Average of midterm and final exam scores can replace the Mastering Chemistry score.

    • Homework Assignments:

    • 11 total assignments, with the lowest score dropped.

    • Consists of:

      • Homework Questions: 50%; due Thursdays by 11:59 PM.

      • Adaptive Follow-Up Questions: 50%; due Sundays, 3 days after.

Lab Information

  • Separate CourseLink site for labs; check for schedules.

  • Lab Manual Cost: $30; increases to $40 after first sales week.

  • Lab Schedule: January 6-10, 9:30 AM - 3:30 PM.

  • Important Dates:

    • Mandatory safety training: January 13 - 17.

    • Bring lab notebooks; lab coat and safety glasses only required on other weeks.

  • Lab Credit Requirements:

    • Minimum of 50% overall course grade.

    • Complete at least 5 out of 8 lab activities.

    • Lab activities include:

    • Attendance at "Wet" labs.

    • Completion and submission of data sheets, post-lab reports.

Lab Safety

  • Student Science Safety I Badge:

    • Required for access to Experiment #1, must show TA badge.

    • If not acquired in F24, complete the course on CourseLink.

  • Course Coordinator: Prof. Lori Jones; contact for academics, accommodations, exams, integrity.

Suggestions for Success

  • Learning Approach:

    • Enjoy the material without focusing solely on grades.

    • Read textbook material prior to lectures.

    • Understand concepts rather than memorization.

  • Tools:

    • Bring a scientific calculator to every class.

    • Utilize the Chemistry Learning Centre for additional help (LIB 360).

  • Supported Learning Groups (SLGs):

    • Schedule and leaders:

    • Deirdre: T & Th 1:30 - 3 PM, Library 109.

    • Alexia: T & Th 3 - 4:30 PM, Library 109.

    • Emma: T & Th 4:30 - 6 PM, Library 109.

    • Rachel: M & W 3:30 - 5 PM, Library 246B.

    • Maya: T & Th 6:30 - 8 PM, Library 109.

  • CourseLink Resources:

    • Announcements, Discussions, Practice Quizzes, Get Ready for First-Year Chem.

Lab Grade Weighting

  • "Wet" Labs:

    • Pre-lab Quizzes: 3%, due before the lab.

    • Post-lab Reports: 12%, usually due one week later.

  • "Dry" Labs:

    • Marking modules: 10% of final grade.

  • Exams:

    • Midterm: February 8, 10 AM; covers Thermochemistry & Thermodynamics (Weeks 1-5).

    • Final Exam: April 8, 8:30 AM; evaluates entire course with focus on post-midterm material.

Course Topics Schedule

  • Thermodynamics: January 6 – February 7.

  • Kinetics: March 17 – April 4.

  • Final Exam: April 8.

Introduction to Thermodynamics and Kinetics

  • Scope of Thermodynamics and Kinetics:

    • Historical development through experimentation and imagination over thousands of years.

    • Accessibility of this deep knowledge within a couple of years of study.

  • Methodology of Learning:

    1. Condensation: Consolidate extensive knowledge into fundamental laws.

    2. Accuracy: Strive for precise measurements to enhance the validity of proposed laws.

    3. Testing Predictions: Conduct new experiments using advanced instruments to formulate new laws.

Importance of Related Sciences

  • Molecular Science:

    • Investigates how molecules change and the rate of those changes.

    • Focuses on the impact of molecular behavior on various life aspects.

  • Material Science:

    • Explores methods for creating new materials and understanding their properties and behaviors.

  • Engineering:

    • Encompasses energy, engine functionality, and industry applications.

Energy Framework

  • Energy Definition: The potential or capacity to move matter; measured in joules (SI unit).

  • Types of Energy:

    • Kinetic Energy (Ek): Energy of motion, defined by the formula:
      E      k = \frac{1}{2}mv^2 where $m$ is mass and $v$ is velocity.

    • Potential Energy (E_p): Energy related to position or configuration.

    • Internal Energy (U): Energy associated with random molecular motion.

Conservation of Energy-Mass

  • First Law of Thermodynamics:

    • States that energy cannot be created or destroyed but can change forms:
      \Delta U = q + w
      where ΔU is the change in internal energy, q is heat added to the system, and w is work done on the system.

System Classifications

  • System Types:

    • Open System: Allows both mass and energy exchange (e.g., open beaker).

    • Closed System: Allows energy exchange but no mass movement (e.g., sealed flask).

    • Isolated System: Neither mass nor energy exchanges occur (e.g., insulated container).

  • Surroundings: Defined as everything else outside the system, collectively known as the 'universe.'

Key Concepts of Heat and Temperature

  • Temperature: A measure of the average kinetic energy of particles within a substance.

    • Higher temperature indicates higher kinetic energy: If T1 > T2, object 1 has higher energy than object 2.

  • Thermodynamic Questions: Examinations include:

    1. How does energy interconvert? How much is involved?

    2. Is a particular reaction feasible at a given temperature?

    3. What is the extent of useful work obtainable from any reaction?

Thermochemistry

  • Defining Thermal Relationships:

    • Encompasses the study of the heat exchange during chemical reactions, where:

    • Exothermic Reaction: Heat is released, leading to an increase in temperature.

    • Endothermic Reaction: Heat is absorbed, resulting in a decrease in temperature.

Practical Exercises

  • Exercise 1: Calculate the kinetic energy of a person weighing 75.0 kg running at 1.78 m/s (use relevant formulas).

Importance of SI Units

  • Unit Consistency: The significance of consistent unit usage is emphasized by a historical incident where NASA lost a Mars orbiter due to a mix-up between metric and English units.

  • Unit Conversion Process: Requires multiplication or division to eliminate unwanted units, retaining only desired units.

Significance of Figures and Uncertainty

  • Significant Figures: Represent measurement accuracy and the effect of experimental errors.

  • Influence of Instrumentation Limits: Variability in instruments affects precision; results must reflect correct levels of significant figures to maintain accuracy.

  • Key Aspects: Precision, estimation, and accurate representation are critical in thermodynamic and kinetic studies.