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Introduction to Chemistry I-Week 7 Notes

by: Lindsey Notetaker

Introduction to Chemistry I-Week 7 Notes CHEM121A

Marketplace > University of Nevada - Las Vegas > Chemistry > CHEM121A > Introduction to Chemistry I Week 7 Notes
Lindsey Notetaker

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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 th...
General Chemistry 1
Dr. Berg
Class Notes
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This 2 page Class Notes was uploaded by Lindsey Notetaker on Saturday October 15, 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 7 views. For similar materials see General Chemistry 1 in Chemistry at University of Nevada - Las Vegas.


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Date Created: 10/15/16
Introduction to Chemistry I-Week 7 Notes (October 10, 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 from 5.4 to the end of chapter 5 (:  Lecture Notes   To find enthalpy problems need to look at how much energy it used through each phrase   For a chemical equation that is balanced, if it is given the change in enthalpy you divide it by the coefficient for the reactants and products to find the heat change   If you switch the reactants and products around then the change in enthalpy becomes the  opposite of the original o Ex. If AX + BY   AY + BX with an change in enthalpy of 347 kilojoules then  AY + BX  AX + BY has a change in enthalpy of ­347 kilojoules   Enthalpy change depends on what state the reactants are in   Hess’s law:  if a reaction is carried out in a number of steps, change in enthalpy for the  overall reaction is the sum of change in enthalpy for each individual step.  Heat of formation is the amount of energy is takes to make one mole of a compound from the reaction of its elements in their most stable forms.  Bond enthalpies are when a bond is broken in the gas form Textbook Notes  To find the enthalpy you can subtract the enthalpy of the reactants from the enthalpy of  the products  Guidelines for using thermochemical equation and enthalpy diagrams  o Enthalpy is an extensive property   This means that it depends on how much there is so if you double the  moles of the reactants then the change in heat will be twice the original  o Enthalpy is the opposite when reactants are switched with the products  o Enthalpy depends on the states of the reactants because some states require less  energy and heat than others  Specific heat= (quantity of heat)/((grams of substance) X (temperature change)) When using a calorimeter to measure the heat transfer, it is important to keep the pressure constant  Vocabulary Words       Enthalpy of Reaction:      Calorimetry:       Calorimeter:       Heat Capacity:  Page 1 of 2 Introduction to Chemistry I-Week 7 Notes (October 10, 2016)      Molar Heat Capacity:       Specific Heat Capacity:  Page 2 of2


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