Lab 10 Lab Report

1 m Lab 10 “Heat Transfer.” Heat is the amount of energy transferred from one high temperature object to a low temperature object. Heat transfer leads to change in temperature of the objects, it drops the temperature of high temperature object and increases that of the low temperature object. This process leads to thermal equilibrium, when the objects have the same temperature. The temperature change of a material depends on their Specific Heat Capacity (c), the amount of energy required to change the temperature of 1? of material, 1 ° 𝐶 . For example, ? 𝑤???? = 4.186 𝐽 = 1 ?𝑎? . The Calorie content in foods are based on 1 𝐶𝑎? = 1000 ?𝑎?. A calorimeter is an apparatus used to study changes in temperature. The calorimeter design permits to isolate the system being studied, heat cannot enter or leave the system from the outside. A thermos, lunch box, or styrofoam cup are all examples of imperfect calorimeters (a sealed styrofoam cup is actually a very good calorimeter, styrofoam is a very good thermal insulator, it is composed of many trap air bubble). In a perfect calorimeter, no energy leaves or enters the system from the outside. In this lab, you will use a calorimeter and the specific heat of water to compare the heat loss of hot water to the heat gain of cold water. The specific heat of a non-perfect calorimeter will be accounted for in the calculations using the specific heat of the metal it is made of. Materials: • Calorimeter • Thermometers • Ice water • Beaker • Hot water • Electronic Balanced • 100 mL Graduated Cylinder PROCEDURE 1. Specific Heat Capacity of water is ? 𝑤𝑎??? = 1 ?𝑎? 2. Specific Heat Capacity of Aluminum ? 𝐴? = 0.22 ?𝑎? 3. Determine the mass of the calorimeter cup: ? ??? = ? 58.15 Part A: Adding Hot water to Cold water. • ? ???+???? 𝑤𝑎??? = ? 157.35 • : ? ???? 𝑤𝑎??? = 99.22 • : ? ???𝑎? = ? 278.27 • : ? ℎ?? 𝑤𝑎??? = 120.92 ? TABLE I: 𝑀𝑎?? (?) Initial Temperature 𝑇 𝑖 (℃) Final Temperature 𝑇 ? (℃) Heat 𝑄(?𝑎?) Cold Water 129.07 g 8.7 °C 43.6 °C 4508.83 Q Calorimeter Cup 58.15 g 8.7 °C 43.6 °C 557.77 Q