Rusch-Lab4.docx

# Rusch-Lab4.docx - CHM130 Lab 4 Calorimetry Name Josef Rusch...

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CHM130 Lab 4 Calorimetry Name: Josef Rusch Data Table: (12 points) ALUMINUM METAL Pre-weighed Aluminum metal sample mass (m metal ) 19.93g Temperature of boiling water and metal sample in the pot (T i(metal) ) 96.1°C Temperature of cool water in the calorimeter prior to adding hot metal sample (T i(water) ) 21.9°C Maximum Temperature of water/metal in calorimeter after mixing (T f ) 27.0°C LEAD METAL Pre-weighed Lead metal sample mass (m metal ) 19.94g Temperature of boiling water and metal sample in the pot (T i(metal) ) 97.9°C Temperature of cool water in the calorimeter prior to adding hot metal sample (T i(water) ) 22.5°C Maximum Temperature of water/metal in calorimeter after mixing (T f ) 23.2°C IRON METAL Pre-weighed Iron metal sample mass (m metal ) 19.95 g Temperature of boiling water and metal sample in the pot (T i(metal) ) 98.1°C Temperature of cool water in the calorimeter prior to adding hot metal sample (T i(water) ) 22.8°C Maximum Temperature of water/metal in calorimeter after mixing (T f ) 24.2°C Calculations (show work for all calculations) Aluminum Sample: 1. Calculate the change in temperature for the water caused by the addition of the aluminum by subtracting the initial temperature of the water from the

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final temperature of the water. ΔT = T f - T i (5 points) The change in temperature for the water caused by the addition of the aluminum is as follows: Ti=21.9°C Tf=27.0°C ΔT= 27.0-21.9 ΔT= 5.1°C change in water temperature 2. Calculate the change in the metal’s temperature by subtracting the initial temperature of the aluminum from the final temperature of the aluminum. ΔT = T f - T i (5 points) The change in the metal’s temperature is as follows: Ti=96.1°C Tf=27.0°C ΔT= 27.0-96.1 ΔT= -69.1°C change in metal’s temperature 3. Determine the mass of the water by using the water’s density (specific to the initial temperature) and the volume of the water. Remember, density = mass/volume . You can look up the density of the water at your specific temperature at htt p :/ / s u.e d u/ c hem i stry/resource/H2Odens i ty_v p. htm l . (5 points) The mass of the water is calculated as follows: Density of water at 21.9°C is 0.9977735g/mL Mass = Density x Volume Mass = 0.9977735g/mL x 75.0mL Mass = 74.8330125g or 74.8g 4. Use the equation: q = m(SH)ΔT to solve for the amount of heat gained by the water from metal. You have the mass of water from calculation #3, the specific heat of water is 4.184 J/g(oC), and the temperature change of water from calculation #1. (10 points) The amount of heat gained by the water from metal is as follows: q = 74.8g x 4.184 J/g(°C) x 5.1°C q = 1596.11232 J or 1600 J heat gained by the water from metal 5. Use the equation: q = m(SH)ΔT to solve for the specific heat of the metal.

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