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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Ten Minutes of Specific Heat Remi Adams East Rowan High School AP Environmental Science Abstract Specific heat and climate were the primary focus of this lab. Specific heat is defined as “the measure of the ability of a substance to change temperature”. The purpose for carrying out this lab was to determine the specific heat/rates of both soil and water‚ and then comparing them. Students also were to relate specific heat to climate. Students were to determine which substance expressed
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Does he successfully explain why so many people died? The heat wave in Chicago 1995 was not only a natural disaster‚ but according to Klinenberg‚ it was a social and political disaster as well. Chicago and its residents were going through an extreme weather condition; it was a combination of heat and humidity and it developed into a massive panic throughout the entire city‚ as people were suffering immensely. Due to the great heat‚ people were searching for alternatives when the electricity and
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Specific heat is the property of the material that an object is made of. The greater the material’s specific heat and the mass‚ the more energy must be added to change its temperature. The goals of this lab were to calculate the specific heat of water and compare to the known value of 4.19J/°Cg. Another goal was to calculate the efficiency of the hot pot used for the experiment and to estimate the cost to heat water for a cup of tea and to bath in a bathtub. The thermal energy E= cm Δ T‚ required
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(MEC 2700) LABORATORY MANUAL JULY 2007 Table of Contents Experiment 1: Heat Capacity of Gases Experiment 2: Thermal and Electrical Conductivity of Metals Experiment 3: Heat Pump Experiment 4: Heat Conduction Experiment 5: Free and Forced Convection Experiment 6: Thermal Radiation Experiment 1: Heat Capacity of Gases 1. BACKGROUND The first law of thermodynamics can be illustrated
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Module 1: Lesson 5 ASSIGNMENT (12 marks) Lesson 5 Assignment Part 1: Molar Heat Calculations (3 marks) 1. Calculate the molar enthalpy of the NaOH(aq) using the data obtained from this experiment. Show all your work. Answer: Specific heat capacity: 4.19 J/g∙°C 50.0 ml of 1.0 mol/L NAOH Initial temperature: 23.9 °C Final temperature: 32.9 °C Change in temperature: 9 °C Q = mc∆t = (80g)(4.19 J/g∙°C)(9°C) = 3016.8 J or 3.0168 kJ ∆rH = n∆rHm 3.0168 kJ = (0.05
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Heat Exchanger Network Design for the Cumene Process | C.A.K.E. Because We’re Just that Delicious Iowa State University Ames IA‚ 50010 | Crego‚ Courtney LHines‚ KirkMonterrubio‚ AmyToohey‚ Erin | Abstract Often a major consideration of a chemical process plant is the high cost of utilities used for heating and cooling of process streams. Heat integration of process streams is an effective way to reduce the cost of these utilities‚ and this process is often referred to as a MUMNE (minimum
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Sameera Raziuddin Latent Heat of Fusion April 11‚ 2011 Abstract: A calorimeter‚ water at room temperature‚ ice‚ and a Pasco GLS Explorer were used in combination with a known value of the latent heat of fusion to create and carry out an experiment to determine the mass of an unknown amount of ice. Using the formula for latent heat of fusion‚ the mass of the ice was calculated to be 45.76g. The error of the carried out experiment was calculated to be 20.06%. Introduction:
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Title: Specific Heat of Solids II. Object: To determine the specific heat capacity of solids by methods of mixtures. III. Theory: When to or more substances at different temperatures are mixed‚ heat will flow from the substance of higher temperature to the substance of lower temperature. The heat flow will continue until equilibrium in temperature is reached. From the Law of Conservation of Energy‚ whatever amount of heat is lost by the hot substance must be equal to the heat gained by the cold
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OPTION A - SIGHT AND WAVE PHENOMENA 1. Standing (or stationary) waves Formation of standing waves : When two identical waves travel along a string in opposite directions (ex : flick a rope attached at the other end)‚ they will superpose and create a standing wave (use animation to visualize what happens). Nodes‚ antinodes. Differences between progressive and standing waves : Wave profile doesn’t progress ; All points between two nodes are in phase (they all reach their maximum at the
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