Exam 4 Flashcards
why study gases?
1) To gain an understanding of real-world phenomena
2) To gain an understanding of how science “works”
gas
- Uniformly fills any container
- Mixes completely with any other gas
- Exerts pressure on its surroundings
- has small forces between them
barometer
- Device used to measure atmospheric pressure
- Mercury flows out of the tube until the pressure of the column of mercury standing on the surface of the mercury in the dish is equal to the pressure of the air on the rest of the surface of the mercury in the dish
- mm Hg
units of pressure
- Unit millimeters of mercury (mm Hg) is often called the torr
a) The units “torr” and “mm Hg” are used interchangeably - Standard atmosphere (atm): A related unit for pressure
- Pascal: SI unit for pressure (Pa)
- PRESSURE = FORCE / AREA
- SI units = Newton/meter2= 1 Pascal (Pa)
- 1 standard atmosphere = 101,325 Pa
- 1 standard atmosphere = 1 atm= 760 mm Hg = 760 torr
Unit millimeters of mercury (mm Hg) is often called the
torr
what 2 units can be used interchangeably?
torr and mm Hg
Standard atmosphere (atm)
A related unit for pressure
formula for pressure
P = force/area
1 atm = __ mm Hg
760
1 atm = __ torr
760
1 atm = __ Pa
101,325
The pressure of the air in a tire is measured to be 28 psi. Represent this pressure in both torr and pascals.
- 9 atm x 760 torr / 1 atm = 1.4 x 10^3 torr
1. 9 atm x 101325 Pa/ atm = 1.9 x 10^5 Pa
The vapor pressure over a beaker of hot water is measured as 656 torr. What is this pressure in atmospheres?
656 torr x 1 atm / 760 torr = 0.863 atm
Robert Boyle’s Experiment
Study of the relationship between the pressure of the trapped gas and its volume
- when u increase P, you decrease V
- ex: pillow
Boyle’s Law Graph
L shaped curve
- pressure and volume
- inversely proportional
Boyle’s Law
- P1V1 = P2V2
- Pressure and volume are inversely related or inversely proportional
- PV = k
- k is a constant for a given amnt of gas at a specific temp
- V= k/p
- T and moles are constant
A sample of helium gas occupies 12.4 L at 23 °C and 0.956 atm. What volume will it occupy at 1.20 atm assuming that the temperature stays constant?
9.88 L
Graphing Data for Several Gases
- It is easier to write an equation for the relationship between volume and temperature if the lines are extrapolated to the origin of the graph
- Use absolute zero for the temperature
- Absolute zero
absolute zero
temperature of −273 °C beyond which matter cannot be cooled
Charles’s Law Graph
V on y axis and T on x axis
- direct relationship
- straight up
Charles’s Law
- V1/T1 = V2/T2
- Direct proportionality between volume and temperature(in Kelvin) represented by the equation known as Charles’s law
- V = bT (b is a proportionality constant)
- K = °C + 273
- 0 K is called absolute zero
- constant pressure and moles
__ K is called absolute zero
0
Suppose a balloon containing 1.30 L of air at 24.7 °C is placed into a beaker containing liquid nitrogen at –78.5 °C. What will the volume of the sample of air become (at constant pressure)?
0.849 L
Avogadro’s Law
- n1/V1 = n2/V2
- Volume and numbers of moles are directly related (constant T and P)
- V = an (a is a proportionality constant)
- constant temp and pressure