PreLab Q1 What is the temperature is assumed of the metal when it is boiling in water?
PreLab Q2 When the metal is transferred from the boiling water to the calorimeter, will there by any loss of energy? If so, where is the energy going?
PostLab Q1 If a metal with a higher specific heat were used, would this raise or lower the final water temperature? Explain.
PostLab Q2 If 50.0 g of water were used instead of 100.0 g of water, would this raise or lower the final metal temperature? Explain.
PostLab Q3 In a calorimetry experiment, a 0.650 g piece of aluminum (specific heat capacity =0.897 J/g K) at a temperature of 93.0 C is placed in a calorimeter. The calorimeter contains 23.8 mL of water at a temperature of 24.0 C. At what temperature will thermal equilibrium be achieved? The heat capacity of water is 4.184 J/g K.
K = C + 273
- qmetal = qwater
- mC∆T = mC∆T
-(0.65)(.897)(Tf-366) = (23.8)(4.184)(Tf-297)
-0.583Tf + 213 = 99.6Tf- 29500
29713 = 100.183Tf
Tf =296.59 K
PreLab Q2 When the metal is transferred from the boiling water to the calorimeter, will there by any loss of energy? If so, where is the energy going?
PostLab Q1 If a metal with a higher specific heat were used, would this raise or lower the final water temperature? Explain.
PostLab Q2 If 50.0 g of water were used instead of 100.0 g of water, would this raise or lower the final metal temperature? Explain.
PostLab Q3 In a calorimetry experiment, a 0.650 g piece of aluminum (specific heat capacity =0.897 J/g K) at a temperature of 93.0 C is placed in a calorimeter. The calorimeter contains 23.8 mL of water at a temperature of 24.0 C. At what temperature will thermal equilibrium be achieved? The heat capacity of water is 4.184 J/g K.
K = C + 273
- qmetal = qwater
- mC∆T = mC∆T
-(0.65)(.897)(Tf-366) = (23.8)(4.184)(Tf-297)
-0.583Tf + 213 = 99.6Tf- 29500
29713 = 100.183Tf
Tf =296.59 K