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Recognizing Data Matrix 2d barcode in C#.NET U Step 4 Review the Knowledge You Need to Score High

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where n is the number of moles of gas and b is a different constant for each gas The larger the gas particles, the more volume they occupy and the larger the b value The attraction of the gas particles for each other tends to lessen the pressure of the gas, because the attraction slightly reduces the force of gas particle collisions with the container walls The amount of attraction depends on the concentration of gas particles and the magnitude of the particles intermolecular force The greater the intermolecular forces of the gas, the higher the attraction is, and the less the real pressure Van der Waals compensated for the attractive force with: 2 2 corrected pressure = P + an /V where a is a constant for individual gases The greater the attractive force between the mol2 2 ecules, the larger the value of a The n /V term corrects for the concentration Substituting these corrections into the ideal gas equation gives van der Waals equation: 2 2 (P + an /V )(V nb) = nRT The larger, more concentrated, and stronger the intermolecular forces of the gas, the more deviation from the ideal gas equation one can expect and the more useful the van der Waals equation becomes
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Experimental
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STRATEGY
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HINT: Make sure the conditions are STP before using 224 L/mol
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Gas law experiments generally involve pressure, volume, and temperature measurements In a few cases, other measurements such as mass and time are necessary You should remember that P, for example, is NOT a measurement; the initial and final pressure measurements are the actual measurements made in the laboratory Another common error is the application of gas law type information and calculations for non-gaseous materials Typical experiments involving these concepts are numbers 3 and 5 in the Experimental chapter A common consideration is the presence of water vapor, H2O(g) Water generates a vapor pressure, which varies with the temperature Dalton s law is used in these cases to adjust the pressure of a gas sample for the presence of water vapor The total pressure (normally atmospheric pressure) is the pressure of the gas or gases being collected and the water vapor When the pressure of an individual gas is needed, the vapor pressure of water is subtracted from the total pressure Finding the vapor pressure of water requires measuring the temperature and using a table showing vapor pressure of water versus temperature In experiments on Graham s law, time is measured The amount of time required for a sample to effuse is the measurement The amount of material effusing divided by the time elapsed is the rate of effusion Most gas law experiments use either the combined gas law or the ideal gas equation Moles of gas are a major factor in many of these experiments The combined gas law can generate the moles of a gas by adjusting the volume to STP and using Avogadro s relationship of 224 L/mol at STP The ideal gas equation gives moles from the relationship n = PV/RT Two common gas law experiments are Determination of Molar Mass by Vapor Density and Determination of the Molar Volume of a Gas While it is possible to use the combined gas law (through 224 L/mol at STP) for either of these, the ideal gas equation is easier to use The values for P, V, T, and n must be determined The temperature may be determined easily using a thermometer The temperature measurement is normally in C The C must then be converted to a Kelvin temperature (K = C + 273) Pressure is measured using a barometer If water vapor is present, a correction is needed in the pressure to compensate for its presence The vapor pressure of water is found in
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