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Lecture

# Experiment #6 - Calorimetry

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Department
Chemistry
Course Code
CAS CH 131
Professor
Andrei Lapets

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10/23/12 Experiment #6 – Calorimetry Calorimetry is the science of measuring heat. Purpose: Measure the heat exchange in various processes. Background: q = heat = mCΔT m = mass of system C = heat capacity ΔT = change in temperature = T ­ T f i q = ΔH (when ΔP = 0) (enthalpy) + ­ MB  (s)eat  ▯M (aq)+ B (aq) salt                            water heat gained by salt = heat lost by solution + heat lost by calorimeter qsystem= ­(qsolutionq calorimeter ΔH  = ­m C  ΔT – C  ΔT system solutiosolution calorimeter ΔH = ΔH systemnsystem Rearranging and substituting… ΔH = ­((M systemT)/m system[(4.18)V solution calorimeter M system molecular weight of salt ΔT = T ­fT i m system mass of salt 4.18 = heat capacity of solution = C solution V solution volume of solution C calorimetercalorimeter constant I. Determining C calorimeter 1) Measure ~50 mL of water. Record the exact volume. 2) Pour water into the calorimeter. Cover with the lid. 3) Record the temperature every 30 seconds until stable. a. stable temperature = T  = T cold water, initCW, i 4) Boil around 120 mL of water. a. can mess up if boil water too early or too long b. need 100­120 mL of boiling water o 5) Assume the temperature of the hot water is 100 C 6) Transfer the boiling water to the calorimeter using heavy gloves (should still  have cold water in it). 7) Cover the calorimeter and agitate it. 8) Record temperature every 30 seconds for 5 minutes agitating throughout.  (Don’t record time at 0 s
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