88-Calor-Probs-Ans

# 88-Calor-Probs-Ans - CALORIMETRY GCHEM I LAB CONCEPT...

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CALORIMETRY GCHEM I LAB CONCEPT PROBLEMS H reaction (J/mole) = Q reaction (J) / reactant (moles) Q reaction (J) = Qsolution (J) Q solution (J) = Q released/absorbed by reaction + Q calorimeter lost/gain Q released/absorbed by reaction = [mass] [specific heat] [ T] Q calorimeter lost/gained = [C] [ T] T ( o C) = Temperature (final) – Temperature (initial) ( sign is important) Specific Heat = Constant Mass Solution = Mass solution in calorimeter (added masses or use density) 1) A solution containing 100.00 grams of water and 6.72 grams of KNO 3 was placed in a calorimeter. The specific heat of the solution was 3.698 joules/gram – o C and the temperature decreased from 19.79-16.41 o C. If calorimeter constant is 82.5 J/ o C, what is heat released/gained by the reaction and heat lost/gained the calorimeter ? Q released/gained by reaction = (mass) * (Specific Heat) * ( T) = (106.72) * (3.698) * (3.38) = 1,327.4 J 1,330 J 3 S/F Q lost or gained by calorimeter = Calorimeter constant) * ( T) = (82.5) * (3.38) = 278.8 J 279 J 3 S/F 2) In a calorimeter 50.0 mls of 1.100 M AgNO 3 and 100.0 mls of 0 1.100 M KCl with a total mass of 180.0 grams are mixed to yield AgCl (s). The reaction increased the temperature in the calorimeter increased from 21.34 to 25.60 o C. If the specific heat of reacting solution was 5.1419 J/gram-

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88-Calor-Probs-Ans - CALORIMETRY GCHEM I LAB CONCEPT...

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