Transcript of 1 Torricelli’s Barometer. 2 A simple manometer for measuring gas pressure in a container.
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Torricelli’s Barometer
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A simple manometer for measuring gas pressure in a container
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Robert Boyle
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A J-tube similar to the one used by Boyle
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Increased pressure leads to decreased volume
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Table 5.1 Actual Data from Boyle's Experiment
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Plotting Boyle's Data
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As pressure increases, the volume of SO2 decreases
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As pressure increases, the volume decreases
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Antoine and Marie Lavoisier(Painting by Jacques-Louis David)
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Empress Eugenie of France(Painting by Franz Winterhalter)
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Prof. Jacques Charles
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Increasing the temperature of a gas (at constant pressure) increases its volume.
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Plots of V versus T(Celsius) for several gases
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Plots of V versus T using the Kelvin scale for temperature
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At constant volume, pressure increases in proportion to Kelvin temperature.
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Boyle’s law: PV = k (for constant T)Charles’s law: V = kT (for constant P)Gay-Lussac’s law: P = kT (for constant V)
COMBINE ALL THREE:
PV = k T or
PV/T = k for any sample
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PV = PVT T
(for any sample of gas under two sets of conditions)
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One mole of any gas at S.T.P. (273 K, 1.0 atm.) occupies 22.4 L and just fits into this box
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At a given temperature and pressure, each of these balloons holds the same number of moles.
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The partial pressure of each gas in a mixture depends on the number of moles of that gas.
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PV = n RT
R = 0.0821 L atm / mol K
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Kinetic molecular theory models gases as large numbers of randomly moving particles of negligible volume that interact with other particles (and container walls) only by collision.
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The End
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The production of oxygen by thermal decomposition of KClO3
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Reaction of zinc with HCl
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Effusion of a gas into an evacuated chamber
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Relative molecular speed distribution of H2 and UF6
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NH3 gas and HCl gas diffuse toward each other and react to form solid NH4Cl
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Velocity distribution of N2 molecules at 3 different temperatures
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Slower Molecules Produce a Lower Pressure
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Gas at low concentration has relatively fewer interactions between particles
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Pairwise interactions among gas particles
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Velocity distribution of O2 Molecules at STP
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The volume taken up by the gas particles themselves is less important (a) at low pressure than (b) at high pressure.
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Molecular Sieve Model
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Inflated Air Bags
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The pressure exerted by the atomsphere can be demonstrated by boiling water in a large metal can
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Acid Rain: Statue in 1990
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Schematic diagram of the process for “scrubbing” sulfur dioxide emissions from
stack gases in power plants
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An environmental officer testing the pH of water.
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Atmospheric composition of dry air near sea level
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Variation of temperature (blue) and pressure (dashed lines) with altitude
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Molar volumes for various gases at 0°C and 1 atm
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Plot of PV versus P for several non-ideal gases at low pressure
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Plot of PV/nRT versus P for Nitrogen gas at 3 temperatures
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Plot of PV versus P for 1 mol of ammonia.
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Plots of PV/nRT versus P for Several Gases (at 200K)
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Values of the van der Waals constants for selectedgases
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Increased volume due to increased moles of gas at constant temperature and pressure
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The ratio of the volumes of gaseous N2 and liquid N2 is 22.4/0.035=640 and the spacing of the molecules is