CHEM103 Lecture Notes - Lecture 9: Calorimetry, Heat Capacity

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emeraldmouse191

26 Sep 2018

School

University of Delaware

Department

Chemistry and Biochemistry

Course

CHEM103

Professor

Chatellier

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Document Summary

Chem test 34 questions - multiple choice - will be given a periodic table. Thermochemistry: is the study of the energy changes that accompany chemical reactions. Calorimetry: is the measurement of the temperature changes that result from these energy changes. Law of conservation of energy: energy is never created or destroyed, changes from one form to another or transferred from one place to another. Q lost = - q gained (start with for any calorimetry problem) Q lost = the amount of heat lost by one object. Q gained = amount of heat gained by another object. Heat capacity: the amount of heat needed to raise an object"s temperature by 1. 00 degrees. Specific heat: the amount of heat needed to raise the temperature of 1. 00 gram of a substance by 1. 00 degree c. Specific heat of water is 1 degree c. *for calculations watch ud capture and section 5. 4 example in book, also found in lecture notes.

Related Questions

Calorimetry is a method used to measure changes inenthalpy, or heat, that occur during chemical processes. Two commoncalorimeters are constant-pressure calorimeters and constant-volume(or "bomb") calorimeters. Bomb calorimeters are used to measurecombustion and other gas-producing reactions, in which the reactionis observed in a strong, sealed vessel. A simple constant-pressurecalorimeter can be made from a foam coffee cup and a thermometer,in which energy changes in a reaction are observed via the changein temperature of the solution in the cup. The idea behindcalorimeters is that if they are sufficiently insulated from theoutside environment, any energy gained or lost in the chemicalreaction will be directly observable as a temperature and/orpressure change in the calorimeter.