Submitted by: Submitted by haruharu1997
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Category: Science and Technology
Date Submitted: 08/28/2015 05:12 AM
CHEM 17 REVIEWER:
CALORIMETRY
Chemical Energy
* contributes to internal energy of a system
Heat of Reaction
* q exchanged when reaction occurs within system at CONSTANT TEMPERATURE
* Exothermic:
* ISOLATED SYSTEM: T INCREASE
NON-ISOLATED SYSTEM: T DECREASE
qrxn < 0
* Endothermic:
ISOLATED SYSTEM: T DECREASE
NON-ISOLATED SYSTEM: T INCREASE
qrxn > 0
Calorimetry
qrxn = -qcal
*qcal = qbomb + qwater + qwires . . .*
qcal = mc ΔT
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qcal = Ccal ΔT
* calibration – establishes a relation bet. quantity value and corresponding measurement
* Bomb Calorimeter
* Coffee-Cup Calorimeter
* system is isolated
* measure ΔT
* standardized using known reaction
1st Law of Thermodynamics
* U – total energy in system
* translational KE (molecule bond)
* molecular rotation (molecule rotates)
* bond vibration (vibrational bond)
* intermolecular attractions
* system contains only U
* heat and work only occur when there is change in system
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ΔU = q + w
Important Equations:
a. 1st Law of Thermodynamics
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qrxn = -qcal
b. Heat of reaction at constant pressure
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qrxn = nLR ΔHrxn
c. Calibration of Calorimeter
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Δ = - Ccal ΔTcal
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nLR
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Ccal = - (nLR * Δ )
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ΔTcal
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d. Determination of Enthalpy Change
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Δ = - [Ccal +( mx cx )] ΔT...