Introduction to Chemistry I-Week 6 Notes (October 3, 2016)
Introduction to Chemistry I-Week 6 Notes (October 3, 2016) CHEM121A
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This 2 page Class Notes was uploaded by Lindsey Notetaker on Thursday October 13, 2016. The Class Notes belongs to CHEM121A at University of Nevada - Las Vegas taught by Dr. Berg in Fall 2016. Since its upload, it has received 23 views. For similar materials see General Chemistry 1 in Chemistry at University of Nevada - Las Vegas.
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Date Created: 10/13/16
Introduction to Chemistry I-Week 6 Notes (October 3, 2016) Chapter 5: Thermochemistry Key to my notes: all notes that are taken from the lecture will be the first section, notes I take from the textbook will be the second section, and the vocabulary words from the chapter with definitions will be the last sections! This is the first part of the chapter 5.1 to 5.3 (: Lecture Notes Energy is the capacity to do work or to transfer heat Work is force X distance o The unit is Joule (1 [kilogram X meters squared]/[seconds squared]) o 1 calorie = 4.185 Joules Heat is thermal energy the energy transferred from a hotter object to a colder object Kinetic energy is half of the mass X velocity First law of thermodynamics is that energy is neither created nor destroyed Change in energy= heat + work = work – pressure X change in volume Enthalpy = energy = pressure X volume Every element has their own specific heat capacity Heat capacity is the amount of energy required to raise the temperature of an object by one degree Molar heat capacity is heat capacity of one mole of a substance Specific heat capacity is the heat capacity of one gram of a substance Heat (q)= mass (m) X specific heat (c or s) X change in temperature If it says change then it has a sign but released, gained, lose, do not have a sign Stopped at IMP TYPES OF ENTHALPY CHANGE Textbook Notes Kinetic energy= ½ (mass X speed squared) Potential energy is “stored” energy and based on position o Electrostatic potential energy is based on interaction of charged particles Electrostatic potential energy= [(constant of 8.99 X 10^9) X (charge of particle 1) X (charge of particle 2)]/(distance of the two particles) Forms of energy can be converted to other forms The SI unit for energy is the Joule o Sometimes convert to calorie which is 1 calorie = 4.184 Joules When studying it is important to know what kind of system you are working with o Open energy and matter can interact with the surrounding o Closed energy and matter cannot interact with the surrounding o Isolated energy and matter do not interact with each other or their surroundings Work=force X distance The change in energy can be found by subtracting the initial internal energy level from the final internal energy level Introduction to Chemistry I-Week 6 Notes (October 3, 2016) o When the total is positive that means that the final internal energy is greater than the initial internal energy meaning the system has gained energy from the surroundings o When the total is negative that means that the final internal energy is less than the initial internal energy meaning the system has lost energy to its surrounding Change in energy = heat + work Vocabulary Words Thermodynamics: Thermochemistry: Energy: Work: Heat: Kinetic Energy: Potential Energy: Joule: Calorie: System: Surrounding: Force: First Law of Thermodynamics: Internal Energy:
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