Looking for a Gas Gas is everywhere. There is something called the atmosphere. That’s a big layer of gas that surrounds the Earth. Gases are random groups of atoms. In solids‚ atoms and molecules are compact and close together. Liquids have atoms that are spread out a little more. Gases are really spread out and the atoms and molecules are full of energy. They are bouncing around constantly. Gases can fill a container of any size or shape. It doesn’t even matter how big the container is. The
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Gas analysis techniques Terms for gas analysis techniques Concentration The term concentration describes the amount of a substance‚ expressed as mass‚ volume‚ or number of particles in a unit volume of a solid‚ liquid‚ or gaseous substance e.g. alcohol in beer or oxygen in air. Different units are in use to describe concentration in gases: Mass concentration Concentration expressed in terms of mass of substance per unit volume [g substance/m3 gas volume] ¢ Volume concentration Concentration
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Introduction A gas is the state of matter that is characterized by having neither a fixed shape nor a fixed volume. Gases exert pressure‚ are compressible‚ have low densities and diffuse rapidly when mixed with other gases. On a microscopic level‚ the molecules (or atoms) in a gas are separated by large distances and are in constant‚ random motion. When dealing with gases‚ the Ideal Gas Law equation is the most famous equation used to relate all the factors in dealing and solving the problem
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Molar Volume of a Gas Objective: The objective is to determine the volume‚ of one mole of hydrogen gas at STP using experimental data‚ known mathematical relationships‚ and a balanced chemical equation. Theory: The goal of this lab is to find the volume of one mole of hydrogen at STP. The experimenters will be working with hydrochloric acid and magnesium to find the objective. The acid in this lab will react to the magnesium and cause the water in the eudiometer to rise because of the reaction
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Lab: Gas Laws Purpose: Obtain a reference of temperatures effect on gas using Charles’ law when heating a capillary tube in water on a heated hot plate. Then‚ cooling the same capillary tube with ice while measuring the temperatures cooling effect on the gas bubble inside the capillary tube. Measurements of temperature change are taken with microLAB sensor and graphed using microLAB software. A final determination of experiments determined absolute zero versus actual absolute zero will be
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Ideal Gas Behavior Author: VanessaStoll Lab Partners: Janelle Vallejo Instructor: Nieves Montano Chem 151‚ Section 002G Date Work Performed: February 12‚ 2014 Date Report Submitted: February 20‚ 2014 Abstract: This paper reports a lab experiment done on the ideal gas law to determine differences in gas based upon their “R” constant difference to 0.082057. A total of seven gases were tested‚ which included‚ Ethanol‚ Hexane‚ Cyclohexane‚ Pentane‚ Ethyl Acetate‚ Butane and Acetone
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The Ideal Gas Law Lab taught me that hydrogen is lighter than air‚ and can be ignited. The materials used for the experiment include 0.05 grams of magnesium‚ 1M H2SO4‚ water‚ a 100mL graduated cylinder‚ and a beaker. The hydrogen can be ignited with a match. First‚ the beaker is filled with water. The acid is then added to the graduated cylinder‚ with about ¾ inch left at the top‚ which is space for water. Afterward‚ the magnesium is added to the graduated cylinder‚ and it is inverted upside down
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How Much Gas CHM 151 LL Wednesday: 11:15-2:00 Instructor: Dr. Leary May 1‚ 2013 Introduction In this project we will choose a solid reagent‚ Mg‚ CaCO3‚ or Na2CO3‚ to react with a hydrochloric acid solution‚ HCl. We are going to measure the amount of gaseous product obtained from the amount of gaseous product obtained from reaction. Then compare to theoretical yield‚ Percent Yield=Actual Yield of Gas/ Theoretical Yield of Gas×100‚ based on stoichiometric prediction. The Ideal Gas Law‚ PV=nRT
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Experiment 3: Evaluation of Gas Constant Purpose: The purpose of this lab is to demonstrate the ideal gas law under ordinary conditions. In this lab‚ the variables in the ideal gas law are known or can be found aside from the constant R. Thus‚ the R values can be found and relatively determine the relevancy of the ideal gas law to the lab conditions. The ideal gas law was tested using the reaction: Mg (s) + 2HCl2 (aq) H2 (g) Procedure: 1. Ribbons of magnesium (5) were cut to the approximate
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Boyle’s Law 5-1: Boyle’s Law: Pressure and Volume Robert Boyle‚ a philosopher and theologian‚ studied the properties of gases in the 17th century. He noticed that gases behave similarly to springs; when compressed or expanded‚ they tend to ‘spring’ back to their original volume. He published his findings in 1662 in a monograph entitled The Spring of the Air and Its Effects. You will make observations similar to those of Robert Boyle and learn about the relationship between the pressure and
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