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18 Cards in this Set
- Front
- Back
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True or false: Gasses expand to to fill their container.
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True.
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Which four variables describe the physical condition of a gas ?
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1. Pressure
2. Volume 3. Temperature 4. Mole |
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What is Boyle's law ?
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The volume of a gas is inversely proportional to its pressure. PV = constant.
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If the temperature and mole of a gas remain constant, with what factor will the volume of a gas increase or decrease if you double its pressure.
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Its volume will decrease with a factor of 0,5.
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What is Charles' law ?
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The volume of a gas is directly proportional to its temperature. V/T = constant.
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What is Avagadro's law ?
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The volume of a gas is directly proportional to the amount of moles.
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What is an ideal gas ?
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A hypothetical gas who obeys the behavior depicted in the ideal gas equation.
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Give the ideal gas equation.
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PV = nRT
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What is the relation between a fixed amount of gas' P,V and T when these variable are changed ?
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(P1V1)/T1 = (P2V2)/T2
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Describe density in terms of the ideal gas equation.
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p = (PM)/(RT)
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Describe Dalton's law of partial pressures.
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Total pressure of a mixture of gases equals the sum of the pressures that each would exert if it were present alone.
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Give the equation for a mole fraction.
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mole fraction = (number of moles of single substance)/(total moles in solution or mixture)
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Give a summary of the kinetic-molecular theory.
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1. Gases are molecules that are in continuous motion
2. The combined volume of gasses is negligible relative to the total volume of the container 3. Attractive and repulsion forces between gas molecules are negligible 4. Average kinetic energy stays the same 5. The kinetic energy is directly proportional to the temperature |
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Describe why pressure decreases if the volume of a gas decreases.
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Because volume decreases the distance that each individual molecule of the gas must travel to collide against the surface of the container is increased. Therefore the frequency of the collisions is decreased and so does the pressure.
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Describe why pressure increases with an increase in temperature.
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When the temperature increases, the average kinetic energy of the molecules of the gas increases, thus the speed of the molecules increases. Therefore the frequency of collisions against the container is increased and so is the pressure.
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In which cases do gases not behave 'ideally' ?
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1. High temperatures
2. High pressures |
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If we talk about a gas as ideal, what factors do we automatically assume ?
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1. That the volume that the molecules themselves occupy are negligible
2. That the attractive and repulsion forces between molecules are negligible |
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Give the van der Waals equation.
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P = [(nRT)/(V-nb)] - [(n^2.a)/V^2)]
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