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CHEM-C127 Calorimetry Lab Notes

by: Kathryn Brinser

CHEM-C127 Calorimetry Lab Notes Chemistry C127

Marketplace > Indiana University > Chemistry > Chemistry C127 > CHEM C127 Calorimetry Lab Notes
Kathryn Brinser
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About this Document

These notes cover the lecture material in preparation for the lab on Calorimetry.
Principles of Chemistry and Biochem I Lab
Dr. Norman Dean
Class Notes
chem-c127, Chemistry, Chem, chem c127, c127, calorimetry, calorimetry lab, calorimetry notes




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This 1 page Class Notes was uploaded by Kathryn Brinser on Sunday February 14, 2016. The Class Notes belongs to Chemistry C127 at Indiana University taught by Dr. Norman Dean in Fall 2016. Since its upload, it has received 68 views. For similar materials see Principles of Chemistry and Biochem I Lab in Chemistry at Indiana University.


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Date Created: 02/14/16
C127 Calorimetry Notes 1-21-16  Learning goals: o Understand energy flow between system and surroundings o Determine specific heat capacity of a metal o Determine enthalpy change of chemical reaction o Determine specific heat capacity of salt solution  Constant pressure and volume in this class; no changes in work  Lab safety: hot plates, acid (HCl), base (NaOH) o Chemical products (says all solutions) can go down sink  Keep in mind Law of Conservation of Energy o Kinetic (thermal) vs. Potential (chemical) energy o Only way system and surroundings interact with each other with exchange of energy  Δ???????????????????????????? = −Δ???? ???????????????? o Δ???? = ???? + ???? o ???? ????????????????????????= −???? ????????????????  ???? = ????????Δ???? o ???? ???????????? ????????????Δ????????????????= −???? ???????????????? ????????????????Δ????????????????????  Ex. ???????????????? + ???????????? → ???? ????2+ ???????????????? o System- reactants and products o Surroundings- water and calorimeter  Calibrating calorimeter o Use same amount of water at all times o Corrects systematic error (calorimeter absorbing some heat); always makes numbers wrong in same “direction”; random error can do both o Equal amounts of hot and cold water- calculate final temp; define hot water as system, cold water + calorimeter as surroundings o Use 2 temperature probes to keep from transferring more heat than should happen  Pay attention to signs; consistently define change in temperatur???? (Δ???? = ???? − ???? ) 


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