Module 11 Flashcards
Define pressure and name the units used to measure it.
Pressure is the force per unit area that a gas exerts on its surroundings. atm, Torr, mmHg, kPa, and Pa
Write Boyle’s law in your own words.
When the temperature stays the same the product of the volume and the pressure will always be the same.
Which of the laws you studied in this module leads to the Kelvin temperature scale?
Charles’ Law
What general rule must a careful scientist follow when extrapolating data?
You can only extrapolate data when the amount of data is large compared to the extrapolation.
What are the properties of an ideal gas?
The molecules (or atoms) that make up an ideal gas must be small compared two the volume available to the gas. The molecules (or atoms) must be so far apart so that they do not attract or repel each other.. The collisions that occur must be elastic (there must be no energy lost)
Under what conditions do gases behave ideally?
When their pressure is near or lower than 1.00 atm and when their temperature is near or higher that 273 K
What is standard temperature and pressure?
273 K and 1.00 atm
Two steel containers of equal volume contain 2 different gases at the same temperature. The first container holds 1.3 moles of N2 gas, and the second containers 1.3 moles of SO3 gas. Compare the pressures of the 2 containers.
They have the exact same pressures.
A liquid’s temperature is lowered from 50 C to 10 C. Did the liquid’s vapor pressure increase, decrease, or stay the same during that time?
Decrease
The mole reaction of nitrogen gas in compressed air is 0.78. If you have 1,000 molecules of compressed air, how many will be nitrogen molecules?
780 will be nitrogen
How do kiloPascals, Millimeters of mercury, and Torrs relate to Atmospheres
1.000 atm = 101.3 kPa = 760.0 mm Hg = 760.0 Torr
What is extrapolation?
it is following an established trend in data even though there is no data available for that region.
What unit do we use for temperature in module 11’s equations?
Kelvin
What is Dalton’s law of partial pressures?
When 2 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.
What does the pressure of an ideal gas depend on?
it depends of the quantity of that gas (not it’s identity)
