Explanation: Because of copper is a good conductor compared to water because the electrons jump from one element to the other more easily in copper than water. MATERIAL Copper tacks, a test tube, a test tube holder, a digital balance, a thermos with ~1 dl cold water, a digital thermometer and an electric kettle (with enough water to cover the element). PROCEDURE: 1: Fill the electric kettle with enough water to cover the heating copper. Also fill the thermos with cold water and the test tube to 50% with copper tacks. 2: First you measure the mass of the copper tacks and also try to get the mass of the water in the thermos as close to 0.1 kg since 1 dl of H20 = 0.1kg H20.
Measuring Specific Heat for Metals Objectives: 1. Hypothesize about the properties of the metal tested and/or the energy transferred. 2. Calculate the specific heat of the metal using your mass and temperature data. 3.
The calorimeter was designed in 1780 by a chemist named Antoine Lavoisier with help from a mathematician by the name of Pierre Simon de Laplace. Now a widespread tool, we will be using the calorimeter, and our knowledge of equations to find the specific heat of zinc and aluminum. OBJECTIVE/GOAL In this experiment we will Measure the mass and temperature of water in a calorimeter Heat a metal sample of a known mass to a specific temperature Calculate the change in water temperature caused by adding the hot metal sample Calculate the specific heat of the metal using your mass and temperature data PROCEDURE 1. Prepare a data table as directed in the Analysis. Safety goggles and lab apron must be worn for the experiment.
A2a. Experimental Design: By using commonly available materials and accurate measuring tools the experiment will allow others to obtain similar results. Connect the multimeter to the two ends of the coil of wire and vary the temperature of the coil of wire. Materials: Precision multimeter to measure resistance Digital timer to measure time periods Multimeter test clips 1000 foot coil of wire (28 gauge) High-precision digital thermometer 1 liter plastic vessel Tap water: Room temperature Ice/Water mix
AP Chemistry P2 Experiment 2: Formula of a Hydrate 9/24/2013 Purpose: Calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate. Procedure: 1) Set up ring stand with ring clamp, clay triangle, crucible with lid, and burner. Adjust the height of the ring stand. 2) Dehydrating Procedures: 3. Measure approximately 1 g of Copper(II) Sulfate Hydrate into the crucible and crucible and lid.
Copper being much less reactive can be easily extracted by heating with various substances to remove its impurities. Copper compounds are heated to react with oxygen and pure copper is left, and can be refined with electrolysis. Copper ores used for commercial production of copper metal are typically chalcopyrite (CuFeS2) and chalcocite (Cu2S), which are sulfides of copper. Due to the low concentration of copper, raw minerals are crushed to small sizes and concentrated by froth flotation. The resulting material is heated with silica (SiO2) in flash smelting to remove the iron as slag.
The term Cp is the specific heat of the material (at constant atmospheric pressure). Different materials have different specific heat values. The units of specific heat are : Joules/gram deg – C. In this lab we will find the specific heat value of Zinc and compare it to accepted values.This will do by heating a mass of Zinc up to the temperature of boiling water and placing the hot metal into a cup of cold water. The thermal energy that the zinc loses goes into heating up the water in the cup. By knowing the starting temperatures and the final temperature of the water and the zinc, the specific heat of Zinc may be easily obtained.
Introduction: The purpose of this experiment is to determine the empirical formula of magnesium oxide formed by the reaction of magnesium with oxygen. To work out formula by the experiment it is necessary to measure the exact masses of each element present in a sample of a compound. Knowing the masses of magnesium and oxygen and its molar masses it is possible to find how many moles of each element is present in the magnesium oxide. The number of moles then can be used to obtain a molar ratio, which gives us the empirical formula of the compound. During the combustion reaction the ribbon of magnesium metal is heated, it reacts with oxygen from the air in a crucible, producing magnesium oxide: magnesium + oxygen → magnesium oxide We measure the mass of magnesium we use for the reaction, and the mass of magnesium oxide produced at the end of it, then we can work out the mass of oxygen that has been combined with the magnesium.
This raises the boiling point. After my apparatus was setup and distillation was begun water had condensates on the top of the fractionating column. This is to be noted since it can slightly affect the boiling point. As the distillation proceeded it was found that my distillation was occurring fairly slowly compared to other students. This issue was resolved with the addition of tin foil around the fractionating column and
Thermodynamics; Conductivity Measurement Summary In this Lab we found that the thermal conductivity stainless steel to be 11Wm/K, the theoretical result is 15W/mK. This result was reasonably accurate with a 26.6% disparity between the results. The graph of the results showed a straight line showing any errors remained constant during the lab. These results are acceptable when potentially large errors are considered. The lab involved determining the thermal conductivity by electrically heating a sample at one end and water cooling it at the other this gives a linear relationship between temperature and distance form the source which may be manipulated to calculate the thermal conductivity of our material.