Airbags are safety features that are designed to save passengers from harm in a head-on collision. Airbags react within milliseconds of a crash, and the folded nylon bag quickly becomes inflated with nitrogen gas. The inflated airbag has the role of being a cushion for passengers and prevents them from hitting into the steering column and dashboard, which can cause painful injuries for passengers. Airbags were invented by John Hetrick in 1953 after Hetrick, his wife and young daughter got
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the material in the gas phase and to see how the ideal gas experiment could apply to the physical. In this the material we used was, a sip-lock plastic bag, a large plastic beaker, thermometry, dry ice, water, and butane lighter. Introduction In this lab, the experiment focused on the relationship between the temperature and pressure of an ideal gas that was dry ice inside the closed container. Therefore, the volume remains constant because the ideal gas was in a closed container. Experiment Procedure
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What makes the ball curve: Soccer players can make the ball curve by applying a Force, kicking, to the ball that is not in the center of the ball itself. When the ball is struck on the side by a player the ball spins while it is moving forward. In the case of the picture below, the soccer ball was struck on the right side of the ball and is spinning counter-clockwise. What causes the ball to actually curve in the air is a difference in the pressures on either side of the soccer ball. On the left
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Methane CH4 = (6.022 x 1023 atoms/mole) = 6.022x1023 atoms of Methane in one mole 6. In this experiment, the pressure (P) was 1 atm, the temperature (T) was 295 K, the volume (V) was 0.150 L, and the number of moles (n)was 6.2 x 10-3 moles. The ideal gas law states that P*V =
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CHM 1101 Introductory Chemistry Dawn Fox Medeba Uzzi August, 2007 Compiled and edited by Medeba Uzzi Authors’ Note This document is an initiative by the authors in an attempt to deal with what they think may be one of the reasons contributing to the relatively high failure rate in the introductory Chemistry course (CHM 1101) at the University of Guyana. It was brought to our attention that many first year students taking CHM 1101 are unable to efficiently cope with the frenetic pace
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Chapter 5—Gases 5.1: Substances That Exist as Gases Air: 78% N2, 21% O2, 1% Other (such as CO2) Ionic compounds do not exist as gases at 25 degrees Celsius as well as 1 atm (due to strong electrostatic forces holding cations/anions together in an ionic solid). The stronger the attractions (intermolecular forces), the less likely the compound can exist as a gas at ordinary temperatures. The characteristics of gases include: assuming the volume/shape of their containers, most compressible
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the number of moles (n)was 6.2 * 10^-3 moles. The ideal gas law states that P*V = n*R*T. Based on your experiment, what value do you get for R? Is your value close to the standard value for R (0.082057 L*atm/K*mol) 7. In a real gas (non-ideal gas) the molecules can interact with each other. If this interaction is attractive, how will the pressure value for this real gas be different than the calcuation of pressure for an ideal
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CHEMISTRY 1031 (CHILDS) – STUDY GUIDE FOR EXAM II Tuesday October 14 BE 160 Exam II will cover the material I lectured on from chapters 4 and 5. You are also expected to retain material from chapters 1, 2, and 3. Everything covered in lecture is fair game for the exam. You will be provided with a periodic table, solubility rules, conversion factors and constants (similar to those at the back of the chapter.) The exam will contain a mixture of multiple choice questions similar to those
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The ideal gas law is where the product of the pressure and the volume of one gram molecule of an ideal gas is equal to the product of the absolute temperature of the gas and the universal gas constant. This is represented by PV = nRT, where R is the ideal gas constant of 0.08206 L*atm/mol*k and is a relationship of energy to quantity of matter at any given temperature. An ideal gas has no definite volume or mass, unlike real gas. Pressure is also higher in ideal gas compared to real gas. Dalton's
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written as V1 = V2 n1 n2 These Balloons Each Hold 1.0 L of Gas at 25 Celsius and 1 atm Increased Volume due to Increased Moles of Gas at Constant Temperature and Pressure 5.3 The Ideal Gas Law Combine the three laws into a single gas law, V = K/P V=K x T V = K x n V = nRT P where R is ideal Gas Constant can be rearranged to, PV = nRT R =
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