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LEAD Data to Accompany Specific Heat of Lead and Aluminum and Lab Report Contents OBSERVATIONS OF THE LEAD SAMPLE: The lead "fishing weight" is a bit difficult to see in the calorimeter in the video so I've taken closer photos to show its color, texture, and overall condition. Recall that your "reference" value for lead is based upon a pure lead sample. The below may have impurities in the form of surface adsorbents, oxidants, etc. Additionally, since it's oddly "fish shaped", I had to use a larger amount of water in the calorimeter to fully cover it. Each gram of water requires 4.18 Joules of heat to get it to raise in temperature by one degree. Therefore using such a large amount of water results in some error because we don't see much of a rise in temperature of the water in the calorimeter.

Specific Heat of Lead and Aluminum: Data and Lab Report Content Dr. Kimberly A. Thomas Revised October 2020 DATA FOR THE LEAD EXPERIMENT: Mass of the lead sample: 229.60 grams Mass of the water in the calorimeter: 237.61 grams Initial temperature of the water in the calorimeter: 23.5 °C Initial temperature of the hot plece of lead: 101.0 °C Final temperature of both the lead and the water (thermal equilibrium): 25.5°C SUPPLED INFORMATION: Actual specific heat of lead (for percent error calculation): 0.128 J/g C Specific heat of water: 4.184 1/g"C *NOTE: I typically do not use "absolute value" signs in the calculation of percent error: Percent Error: Experimental value-actual value x 100 actual value It is therefore possible for you to get a percent error with a negative sign in front of it. The accuracy of your experiment is just the percentage (without the negative sign) but the negative sign is helpful if you get one because it tells you there. was some heat unaccounted for. In other words, heat loss prior to being "captured" in the water in the calorimeter.

80% OBSERVATIONS OF THE ALUMINUM SAMPLE AND DATA TO ACCOMPANY THE ALUMINUM EXPERIMENT: 27.152 Percent Error: Mass of the aluminum sample: grams Mass of the calorimeter (nested foam cups): 13.827 grams Mass of the calorimeter and water: 80.603 grams Mass of the water: Initial temperature of the water in the calorimeter: 23.3 °C Initial temperature of the hot piece of aluminum: 99.7°C Final temperature of both the aluminum and the water (thermal equilibrium): 29.6°C SUPPLIED INFORMATION: Actual specific heat of aluminum (for percent error calculation): 0.900 1/g°C Specific heat of water: 4.184 1/gC grams (you will determine this by subtraction) *NOTE: I typically do not use "absolute value signs in the calculation of percent error: & Experimental value-actual value x 100 actual value it is therefore possible for you to get a percent error with a negative sign in front of it. The accuracy of your experiment is just the percentage (without the negative sign) but the negative sign is helpful if you p one because it tells you there was some heat unaccounted for. In other words, heat loss prior to being "captured in the water in the calorimeter.

YOUR LAB REPORT FOR SPECIFIC HEAT FOR Pb AND AI SHOULD INCLUDE (be sure to limit answers to the proper number of significant figures): 1. WORKED OUT NEAT, LEGIBLE CALCULATION FOR THE SPECIFIC HEAT OF LEAD 2. PERCENT ERROR CALCULATION FOR THE SPECIFIC HEAT OF LEAD RELATIVE TO ITS ACTUAL SPECIFIC HEAT OF 0.128 1/g °C 3. WORKED OUT NEAT, LEGIBLE CALCULATION FOR THE SPECIFIC HEAT OF ALUMINUM 4. PERCENT ERROR CALCULATION FOR THE SPECIFIC HEAT OF ALUMINUM RELATIVE IT ITS ACTUAL SPECIFIC HEAT HEAT OF 0.900 J/g°C 5. CONCLUSION AND ERROR ANALYSIS: *STATE WHETHER THE GOAL OF THE EXPERIMENT(S) WAS ACHIEVED *DISCUSS THE ACCURACY OF EACH RESULT. WHICH WAS MORE ACCURATE AND WHY? *DISCUSS POSSIBLE ERRORS. THESE ARE THINGS THAT DID GO WRONG OR COULD HAVE GONE WRONG OR IMPACTED THE RESULTS OBTAINED. INCORPORATE THE SAMPLE CONDITION, EQUIPMENT USED, AND METHODOLOGY.