Calorimetry Chemistry 1412 Spring 2013 Objective: Determine the calorimeter constants in a coffee cup calorimeter‚ then the calorimeter will used to determine the quantity of heat that flows in a few physical and chemical processes. Materials used: Choice I: Choice II: * Safety Goggles Safety Goggles * Distilled water Distilled water * 150 mL beaker 600 mL beaker * 50 mL graduated cylinder 50 ml graduated cylinder * Calorimeter Calorimeter
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Data collection and processing Qualitative observation Before * Blue solution of copper sulfate * Grey zinc powder During * Blue color solution changes to greyish black * Heat is given out‚ so the surroundings become hotter. After * Grey powder remains on the sides of the cup * Precipitate formed at the bottom of the cup List of chemicals and apparatus used Chemicals used Copper sulfate solution‚ 1 mol dm-3 25g of zinc powder Apparatus needed
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CHM130 Lab 4 Calorimetry Name: Data Table: (12 points) ALUMINUM METAL Pre-weighed Aluminum metal sample mass (mmetal) 20.09 g Temperature of boiling water and metal sample in the pot (Ti(metal)) dsdfa(Ti 99°C Temperature of cool water in the calorimeter prior to adding hot metal sample (Ti(water)) 24°C Maximum Temperature of water/metal in calorimeter after mixing (Tf) 28°C LEAD METAL Pre-weighed Lead metal sample mass (mmetal) 20.03g Temperature of boiling water and metal sample
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sure to look over all your notes and be sure to know the following things) 1. Define Temperature‚ thermal energy and heat. 2. A 1.00 x 10²g mass of tungsten at 100°C is placed in 2.00 x 10²g of water at 20.0°C. The mixture reaches equilibrium at 21.6°C. Calculate the specific heat of tungsten. Cw = 4180 J/kg°C C= 171 J/kgOC 3. A certain metal has a specific heat of 400 J / kg oC. It absorbs 8000 J of thermal energy which causes its temperature to raise 10oC. How much mass of the metal
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Ocean County College Department of Chemistry Lab 3 Caloric Content of Food Submitted by Juan C. Delgado Román Student # 0439722 Date Submitted: October 26‚ 2014 Date Performed: October 25‚ 2015 Lab Section: Chem-180 Course Instructor: Lea Stage Purpose On this experiment we will learn how measure the energy content of 3 food items and become familiar with energy units: joules‚ and calories
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CHM130 Lab 4 Calorimetry Name: Conor Westerman Data Table: (12 points) ALUMINUM METAL Pre-weighed Aluminum metal -100 grams sample mass (mmetal) Temperature of boiling water and metal sample in the pot (Ti(metal)) 365k and 345k Temperature of cool water in the calorimeter prior to adding hot metal sample (Ti(water)) 364k Maximum Temperature of water/metal in calorimeter after mixing (Tf) 365k LEAD METAL Pre-weighed
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DP Physics IA Thermal physics: Specific Heat Capacity of Metals Introduction: In this experiment we are going to measure the specific heat capacity of a unknown metal. To measure the specific heat capacity we will heat up the metal to certain temperature and release the metal in beaker filled with water. By knowing the mass and temperature of water filled in beaker‚ we will be able to calculate the specific capacity of unknown metal by change in temperature of beaker willed
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Experiment 1 The Heat Capacity Ratio of Gases Purpose The purpose of this experiment is to calculate the heat capacity ratio of gases‚ Helium‚ Nitrogen and Carbon Dioxide‚ and compare with their theoretical values. Introduction Thermodynamics is the study of heat as it relates to energy and work. There are various properties which all relate to each other when determining the characteristic of a certain substance. One of such properties is heat capacity‚ which is the amount of heat energy required
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energy. Planning We will be using 6 different fuels to heat up 100ml of water‚ and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes‚ and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula: Mass of water x 4.2 (water’s specific heat capacity) x temperature change = energy transferred from the fuel
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CHEMICAL Sodium Hydroxide (NaOH) PROCEDURE The recommended amount of compound ito use is around 0.1 moles. Add water into your caleriometer Add the solid salt and stir the mixture thoroughly and continuously. Calculate ΔHsol. Ignore the heat capacity of the caleriometer. _Results_ RAW DATA Tab.1. The different data required for the calculations. Trial Mass of NaOH / g (± 0.001 g) Volume of H2O / ml (± 1 ml) Initial Temperature / °C (± 1 °C) Final Temperature / °C (± 1 °C) 1
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