Title: Specific Heat Capacities of Metals Experiment Date: 3/28/2012 Report Date: 4/4/2012 Purpose: The purpose of the lab is to measure the specific heat capacities of aluminum‚ steel and brass. Theory: The amount of heat (ΔQ) required to change the temperature of an object is proportional to the mass (m) of the object and the temperature change (ΔT) of the object. ΔQ= cmΔT where c is called as the specific heat capacity of the material. In the calorie units system the unit of quantity
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Experiment no. 1 Group No./Time/Day:6/7:30-10:30/Wednesday I. Title: Specific Heat of Solids II. Object: To determine the specific heat capacity of solids by methods of mixtures. III. Apparatus: Lead and Iron shots‚ Electric heater‚ Calorimeter‚ Dipper‚ 2 Thermometers‚ Water bath‚ Set of Masses‚ Trip Scale balance‚ Extension cords
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Marybeth Brooks Physics Lab III Specific Heat Capacity Lab May 25‚ 2011 Abstract The specific heat capacity of various metals can be calculated and compared to accepted literature values. Dropping heated metal samples into a calorimeter filled with water and then measuring the change in the temperature of the system accomplished this. The metal samples were heated in a boiling water bath and were assumed to be at 100 C when they were removed. It was added to a calorimeter and stirrer
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Investigation 11 Specific heat capacity Aim: Investigate to determine the specific heat capacity of a metal cube provided Apparatus: -thermometer -stirrer -water -calorimeter -beam balance -metal cube -beaker Procedure: Using the normal equipment for Thermal Physics investigations‚ you are required to design and carry out an investigation to determine the specific heat capacity of a metal cube provide by teacher. Furthermore‚ you will need to compare your obtained value with
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Specific Heat of a Metal Post-Lab I. Purpose The purpose of this lab is to determine the specific heat of an unknown metal. II. Safety Wear goggles and lab apron at all times. Use caution when boiling water. Do not pick up hot beaker or hot metal with hands. Use tongs. III. Pre-Lab Questions 1. A 12.5 g metal is raised to 100C in boiling water. It is put into 82.8 g of water at 22.4C‚ and the water rises to 28.6C. Recalling that the specific heat of water is 4.18J/gC‚ use the equation above
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Aim: i) To find the relationship between supplied energy and change in temperature of water. ii) To find the specific heat capacity (SHC) of water. Hypothesis: As time increases so does the temperature since the water is exposed to the heated wire for a longer period of time. Variables: The Dependent Variable is the temperature of the water‚ and since the Energy is calculated using temperature it is a dependent variable as well. The constant variables are the voltage and current. Theory:
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for the specific heat capacity of the metal were about .0500 J/mol. This is a large deviation‚ with both of these values identifying very different metals. The average heat capacity identified the metal used as brass. The average heat capacity calculated was .3776 J/mol and the actual heat capacity of brass is .375 J/mol. The second run displayed the closest value to the actual value. A source of error that may have caused a large divide in the calculations could have been when the metal was transferred
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Honors Laboratory: Specific Heat and Conservation of Energy When energy in the form of heat Q is added to a material‚ the temperature of the material rises. Note that temperature‚ in units of degrees Celsius (°C) or Kelvin (K)‚ is a measure of how hot or cold a substance is‚ while heat‚ in units of joules (J) or calories (cal)‚ is a measure of its thermal energy. 1cal = 4.19J. A measure of the efficiency with which a substance can store this heat energy is known as specific heat capacity‚ or simply the
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the experiment aimed to determine the specific heat of two different metals‚ Lead and Zinc‚ in order to calculate their individual atomic weight. Theory The calorimeter consists of a metal outer cup‚ a removable metal inner cup‚ which is held in place by a rubber ring‚ and an insulating lid with a small opening for a thermometer. It is a closed system as the air between the inner cup and outer cup insulates the water and heated metal‚ so‚ ideally‚ all heat is contained within the calorimeter (1)
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vibrating around‚ the hotter the object feels. We can sidestep this molecular picture by dealing with objects as a whole‚ and treating the energy transfer as the flow of heat‚ rather than kinetic energy transfer among particles. |Specific Heat for Various Materials | |Material |Specific Heat | | |(J/kg C°) | |Water |4186 | |Aluminum |900
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