5.0 part 2: calorimetry - mr. mcbride's 4u...
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5.0Part2:Calorimetry
Tostudyenergychanges,weneedanisolatedsystem(noenergycanmoveinorout).Wecallthistypeofsystemacalorimeter.
Theprocessofpreciselymeasuringenergychangesinsidethissystemiscalledcalorimetry.
Oftenforsimplelaboratoryexperiments,asimple,lowcostcalorimeteriscreatedandused.
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Energyistransferredbetweenthechemicalsystemandthewater(knownasthesurroundings).
Thechangeinenergy(H)ofthechemicalsystemisequaltothequantityofheattransferredtothesurroundings,q.(i.e.,whatoneloses,theothergainsandviceversa.)
H=q(chemicalsystem)(calorimeter)
Theenergychangeofthechemicalsystem,H,dependsontwoquantities:
themassofthechemical(Ifyouhavemoremethanetoburn,moreenergywillbetransferred.)
Theenergyconstantforthechangeoccuring,whichiscalledspecificheat,h.ThisquantityhasunitsofJ/g.(Assumingyouburn1gramofpropane,itmaygiveoffmoreheatthanonegramofmethane.Therefore,propanewouldhaveahigherspecificheat.)
H=mh
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Ourequationsthusfar:
SinceH=qandweknowfromyesterdaythatq=mcT,thenH=mcT.
Example1Inacalorimetryexperiment,astudentdissolvessomepotassiumchloride,KF,in100mlofwaterandthetemperaturechangesfrom22oCto18.5oC.IfthespecificheatofsolutionforKFis5.72kJ/g,howmuchKFwasdissolvedinthesolution?
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BombCalorimetersandHeatCapacity
Manychemicalreactionsofinteresttochemistsdonottakeplaceinaqueoussolutions,likecombustion,forexample.Oilcompaniesarealwaysresearchingbettergasolines,andoneimportantcharacteristicofgasolineistheheatreleasedduringcombustion.Acalorimetermadeofstyrofoamcantbeusedtostudytheenergychangesofcombustionreactions.Soweneedsomethingelse.
Westudythesetypesofreactionsinabombcalorimeter.
Readpage578ofyourtextbookandusetheblankspaceprovidedtomakenotesontherelevantinformationyoudiscover.(Youshouldbeworkingtowardsdevelopingtheformulaq=CT.)
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Example2Anoxygenbombcalorimeterhasaheatcapacityof6.49kJ/oC.Thecompletecombustionof1.12gofacetyleneproducesatemperaturechangefrom18.60oCto27.15oC.Calculatethespecificheatofcombustion,hc,foracetylene,C2H2(g).
Homework:pg579#11,12pg581#2,3CalorimetryPracticeQuestions
Therefore, The specific heat of combustion for acetylene is -49.5kJ/g.
Surroundings Chemical System
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Solutions12.2AExtraPracticeQs.pdf
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1. A student reacted a sodium hydroxide solution containing 12.0 g of solute with excess, dilute sulfuric acid. Both solu-tions were initially at 19.67C. The highest temperature reached by a 300.0 mL mixture was 34.06C. Calculate the spe-cific heat of neutralization for sodium hydroxide.
E qNaOH (calorimeter)
mhn mct
12.0 g hn 300.0 g g4.
18C
J (34.06 19.67)C
hn 1.50 kJ/g
The specific heat of neutralization for sodium hydroxide is an exothermic 1.50 kJ/g.
2. Acetylene has a specific heat of combustion of 49.5 kJ/C. Find the temperature increase expected for 1.00 kg of water inthe combustion of 1.45 g of acetylene.
E qC2H2 (calorimeter)
mhn mct
1.45 g 49.
g5 kJ 1.00 kg
g4.
18C
J t
hn 1.50 kJ/g
3. Combustion of 3.50 g of ethanol in a bomb calorimeter with a heat capacity of 15.2 kJ/C causes a temperature increasefrom 19.88C to 26.18C. Using this evidence, determine the specific heat of combustion for ethanol.
E qethanol (calorimeter)
mhc ct
3.50 g hc 15.
2C
kJ (26.18 19.88)C
hc 27.4 kJ/g
The specific heat of combustion for ethanol is an exothermic 27.4 kJ/g.
4. A reference gives the specific heat of combustion of methane as 50.0 kJ/C. What minimum mass of methane must beburned to warm 4.00 L of water from 22.4C to 87.6C, assuming no heat losses.
E qCH4 (calorimeter)
mhn mct
m 50.
g0 kJ 4.00 kg
g4.
18C
J (87.6 22.4)C
m 21.8 g
12.2B
Solutions for 12.2A Extra Practice Questions: Calorimetry
5-22 Unit 5 Lab and Study Masters Copyright 2002 Nelson Thomson Learning
SMART Notebook
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Attachments
Solutions12.2AExtraPracticeQs.pdf
HeatTransfer.mov
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1. A student reacted a sodium hydroxide solution containing 12.0 g of solute with excess, dilute sulfuric acid. Both solu-tions were initially at 19.67C. The highest temperature reached by a 300.0 mL mixture was 34.06C. Calculate the spe-cific heat of neutralization for sodium hydroxide.
E qNaOH (calorimeter)
mhn mct
12.0 g hn 300.0 g g4.
18C
J (34.06 19.67)C
hn 1.50 kJ/g
The specific heat of neutralization for sodium hydroxide is an exothermic 1.50 kJ/g.
2. Acetylene has a specific heat of combustion of 49.5 kJ/C. Find the temperature increase expected for 1.00 kg of water inthe combustion of 1.45 g of acetylene.
E qC2H2 (calorimeter)
mhn mct
1.45 g 49.
g5 kJ 1.00 kg
g4.
18C
J t
hn 1.50 kJ/g
3. Combustion of 3.50 g of ethanol in a bomb calorimeter with a heat capacity of 15.2 kJ/C causes a temperature increasefrom 19.88C to 26.18C. Using this evidence, determine the specific heat of combustion for ethanol.
E qethanol (calorimeter)
mhc ct
3.50 g hc 15.
2C
kJ (26.18 19.88)C
hc 27.4 kJ/g
The specific heat of combustion for ethanol is an exothermic 27.4 kJ/g.
4. A reference gives the specific heat of combustion of methane as 50.0 kJ/C. What minimum mass of methane must beburned to warm 4.00 L of water from 22.4C to 87.6C, assuming no heat losses.
E qCH4 (calorimeter)
mhn mct
m 50.
g0 kJ 4.00 kg
g4.
18C
J (87.6 22.4)C
m 21.8 g
12.2B
Solutions for 12.2A Extra Practice Questions: Calorimetry
5-22 Unit 5 Lab and Study Masters Copyright 2002 Nelson Thomson Learning
SMART Notebook
SMART Notebook
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