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### 32 Cards in this Set

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 the amount of gas in the system is expressed in terms of the number of moles the volume occupied by a gas at a specified temperature and pressure must depend on the number of gas particles the number of moles of gas is directly proportional to the number of particles moles must be directly proportional to volume PV/Tn shows that (PxV)(Txn) is a constant and holds for ideal gases a gas behaves ideally if it conforms to the gas laws has the value 8.31 (L x Kpa)/(K x mol) ideal gas constant (R) P x V = n x R x T R = P x V / T x n ideal gas law what is an advantage of the ideal gas law over the combined gas law it permits you to solve for the number of moles of a contained gas when p,v, and t are known a gas that follows the gas laws at all conditions of pressure and temperature is a truly ideal gas the particles of a truly ideal gas would have no volume and could not be attracted to each other at all is there any gas that is a truly ideal gas no an ideal gas does not exist real gases can behave as ideal gases what is an important behavior of real gases that differs from that of a hypothetical ideal gas real gases can be liquefied and sometimes solidified by cooling and by applying pressure you can analyze how much a gas departs from ideal behavior by considering PVNRT according the ideal gas law, this ratio fr an ideal gas equal 1 by: dividing both sides of the ideal gas lawby nRT PVNRT plotted against pressure gives a _________ for an ideal gas because the ratio is constant horizontal line for real gases at high pressure, the ratio PVNRT may depart widely from the ideal constant value of 1 the explanations for these departures of deviations rom the ideal is based on two factors: the attractions between molecules and the volume of gas molecules PVNRT may be greater or less than one if positive - negative - above the line, below the line simple kinetic theory assumes that gas particles are not attracted to each other and that the paticles have no volume are the assumptions of the simple kinetic theory correct no, incorrect gases and vapors could not be liquefied if there were no attractions between molecules real gases are made up of actual physical particles, which do have volume the intermolecular forces that tend to hold the particles in a gas together effectively reduce the distance between particles the gas occupies less volume than is expected by the no-attractions assumption of the kinetic theory, which causes the ratio to tend to be less than 1 the molecules occupy some volu,e thus contradicting the zero volume assuption of kinetic theory, which causes the ratio to be greater than 1 in portion of the curves below the line, the intermolecular attractions dominate causing the total volume to be less than ideal in portions of the curves above the line, the effect of volume of the molecules dominates, causing the total value to be greater than ideal the ratio is nearly equal to 1 at lower pressure at the elevated temperature the ratio increases to greater than 1 only when the volume of the individual gas paritlces becomes important, as it does at high pressure