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25 Cards in this Set
- Front
- Back
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Pressure
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The force per unit area exerted on an object.
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Charles's Law
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At constant pressure, the temperature and volume of a gas are linearly proportional.
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Extrapolation
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Following an established trend in the data even though there is no data available for that region.
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When using any equation in the module you must always use
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the Kelvin temperature scale
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Standard Temperature and Pressure
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STP- a temperature of 273 K and a pressure that is near( or lower than) 1.00 atm will behave in an ideal fashion.
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Dalton's Law of partial Pressures
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When two or more ideal gases are mixed together, the total pressure of the mixture is equal to the sum of the pressures of each individual gas.
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Where Pt is the total pressure of the gas, and p1, P2, etc. are the pressures due to each individual gas it is called
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partial pressures
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The pressure of an ideal gas does not depend on the identity of the gas, it depends on
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the identity of the gas. It depends ONLY on the quantity of that gas.
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Vapor pressure
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The pressure exerted by the vapor which sits on top of any liquid.
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Boiling point
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The temperature at which the vapor pressure of a liquid is equal to normal atmospheric pressure.
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mole fraction
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a concentration unit that is always used in the context of a mixture
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Pressure
|
The force per unit area exerted on an object.
|
|
|
Charles's Law
|
At constant pressure, the temperature and volume of a gas are linearly proportional.
|
|
|
Extrapolation
|
Following an established trend in the data even though there is no data available for that region.
|
|
|
When using any equation in the module you must always use
|
the Kelvin temperature scale
|
|
|
Standard Temperature and Pressure
|
STP- a temperature of 273 K and a pressure that is near( or lower than) 1.00 atm will behave in an ideal fashion.
|
|
|
Dalton's Law of partial Pressures
|
When two or more ideal gases are mixed together, the total pressure of the mixture is equal to the sum of the pressures of each individual gas.
|
|
|
Where Pt is the total pressure of the gas, and p1, P2, etc. are the pressures due to each individual gas it is called
|
partial pressures
|
|
|
The pressure of an ideal gas does not depend on the identity of the gas, it depends on
|
the identity of the gas. It depends ONLY on the quantity of that gas.
|
|
|
Vapor pressure
|
The pressure exerted by the vapor which sits on top of any liquid.
|
|
|
Boiling point
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The temperature at which the vapor pressure of a liquid is equal to normal atmospheric pressure.
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The vapor pressure of any liquid increases with increasing temperature.
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vapor pressure
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mole fraction
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a concentration unit that is always used in the context of a mixture
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The ideal gas relates the number of moles of a gas to things that are easy to measure. PV=nRT
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ideal gas
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Ideal gas constant is relatively important quantity in the study of chemistry.
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ideal gas
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