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| relationship between volume and pressure. At constant temperature, the volume occupied by a gas is inversely related to its pressure. |
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| relationship between volume and temperature; at a constant pressure, the volume occupied by a fixed amount of gas is directly proportional to its absolute temperature |
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| relationship between volume and amount; at fixed temperature and pressure, equal volumes of any gas contain an equal number of particles. |
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| standard temperature & pressure; 0 deg C (273 K) and 1 atm (760 torr) |
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| 22.414 L; liters that 1 mol of gas occupies at STP |
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| Density formula using ideal gas law. |
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| d=(Molar Mass*Pressure)/(R*Temperature) |
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| Density formula using ideal gas law. |
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| d=(Molar Mass*Pressure)/(R*Temperature) |
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| Molar mass formula(s) using ideal gas law. |
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| Total gas pressure in a container equals the combined pressure of all gases. The partial pressure of a gas is proportioned by its molar fraction in the mixture. p1=x1 * ptotal, where x1 is the mole fraction. |
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Lighter gases effuse faster; the rate of effusion of a gas is inversely proportional to the square root of its molar mass. Rate of effusion~1/sqrt(M).
(rate A/rate b)=(sqrtB/sqrtA) |
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| process by which gas escapes from its container through a tiny hole into an evacuated space |
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| the movement of one gas through another |
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| the ease with which the electron cloud of a particle can be distorted |
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| Strongest intermolecular force; occurs only between H and N, O, or F. |
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| Higher the vapor pressure |
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| Weaker the attractive forces |
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| Weaker intermolecular forces |
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| stronger intermolecular forces |
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| Heat of vaporization increases as |
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| intermolecular forces increase |
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| Ionic compounds have change in EN values |
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| Polar compounds have change in EN values between |
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| A low melting point suggests that ionic bonding |
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