measure the hydrogen gas given off in the reaction of the zinc on the nail and the hydrochloric acid. A Erlenmeyer flask was used to hold the acid and nail which released the hydrogen into a rubber tubing that was fed into a 100 mL graduated cylinder full of water. As the hydrogen entered the upside down cylinder‚ it displaced the water‚ and the volume of gas was measured (gasometric analysis). The ideal gas law was then used‚ PV = nRT. Since the volume‚ temperature‚ gas constant (R)‚ and pressure
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neon (Ne)‚ argon (Ar)‚ krypton (Kr)‚ xenon (Xe) and radon (Rn) ; are called "elemental gases". Alternatively they are sometimes known as "molecular gases" to distinguish them from molecules that are also chemical compounds. Etymology The word gas is a neologism first used by the early 17th-century Flemish chemist J.B. Van Helmont.[4] Van Helmont’s word appears to have been simply a phonetic transcription of the Greek word χάος Chaos – the g in Dutch being pronounced like ch in "loch" – in which
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Jennifer Jiang Dr. Iobst Chemistry I Honors 11 March 2013 Molar Mass of Butane: Applying the Gas Laws 1. Water bath temperature: 17.7° C or 291 K Celsius to Kelvin temperature conversion: 17.7° C + 273 = 290.7 Kelvin (rounded to SF= 291 K) 2. 1 atm 1 atm 10 mm 10 mm 2.54 cm 2.54 cm According to the digital barometer our teacher provided‚ the barometric pressure in the lab is 29.77 in Hg‚ which will need to be converted to atmospheric pressure. 760 mm Hg 760 mm Hg 1 cm
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05.09 Module Five Review and DBA 05.01 Four Phases of Matter * Matter exists in different phases‚ also called states‚ which include solid‚liquid‚ gas‚ and plasma. These phases can be distinguished at the molecular level by how the particles are held together. * Solids * In the solid phase‚ the intermolecular attraction between particles of matter is strong enough to hold all the particles together in a fixed three-dimensional arrangement. Because of the rigid arrangement of particles
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ABSTRACT This experiment was carried out to determine the relationship between the pressure and the temperature of saturated steam in equilibrium. Besides that this experiment was also done to demonstrate the vapor pressure curve. The marcet Boiler was used for this experiment. When the pressure increases‚ the temperature also increases. Therefore‚ the relationship of pressure and temperature is directly proportional. The derived formulae and the data were used to calculate the slope. The dT/dP
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05_CTR_ch14 7/12/04 8:13 AM Page 351 Name ___________________________ 14.3 Date ___________________ Class __________________ IDEAL GASES Section Review Objectives • Compute the value of an unknown using the ideal gas law • Compare and contrast real and ideal gases Vocabulary • ideal gas constant (R) • ideal gas law Key Equation • Ideal gas law: P V n R T or PV nRT Part A Completion © Pearson Education‚ Inc.‚ publishing as Pearson Prentice Hall. All rights
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densities than liquids and solids. NO2 gas 4 Force Pressure = Area (force = mass x acceleration) Units of Pressure 1 pascal (Pa) = 1 N/m2 1 atm = 760 mmHg = 760 torr 1 atm = 101‚325 Pa Barometer For measuring atmospheric pressure 5 The force experienced by any area exposed to Earth’s atmosphere is equal to the weight of that column of air above it. 10 miles 0.2 atm 4 miles Sea level 0.5 atm 1 atm 6 Manometers Used to Measure Gas Pressures closed-tube open-tube Patm
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5.2 Know Boyle’s Law and its assumptions. Boyle’s Law is a principle which says for relatively low pressures‚ the pressure of an ideal gas kept at constant temperature varies inversely with the volume of the gas. It describes the inversely proportional relationship between the absolute pressure and volume of a gas‚ if temperature if kept at a constant. Know Charles’s Law and its assumptions. Charles’s Law (also known as the law of volumes) is an experimental gas law which describes how
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First Law-Exercise: Problem 1: A volume 10 m3 contains 8 kg of oxygen at a temperature of 300 K. Find the work necessary to decrease the volume to 5 m3‚ (a) at a constant pressure and (b) at constant temperature. (c) What is the temperature at the end of the process in (a)? (d) What is the pressure at the end of process in (b)? (e) Show both processes in the p-V plane. Problem 2: The temperature of an ideal gas at an initial pressure p1 and volume V1 is increased at constant volume until the pressure
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general case of a gas‚ liquid‚ or solid‚ the volumetric coefficient of thermal expansion is given by The subscript p indicates that the pressure is held constant during the expansion‚ and the subscript "V" stresses that it is the volumetric (not linear) expansion that enters this general definition. In the case of a gas‚ the fact that the pressure is held constant is important‚ because the volume of a gas will vary appreciably with pressure as well as temperature. For a gas of low density this
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