Chapter 13
Solids: have a definite shape and volume
Liquids: have a definite volume but assumes the shape of the container
Gases: have no definite shape
Liquids and gases are considered fluids
Boyle’s Law: states that the volume of a given amount of gas is inversely proportional to its pressure (at constant temperature): PV=k or P=k/V. As pressure increases, volume decreases.
http://www.iun.edu/~cpanhd/C101webnotes/gases/boyleslaw.html
Atmospheric pressure
Charle's law
These three laws can be combined into the ideal gas law, PV=nRT, where R is called the universal gas constant.
This equation makes it possible to calculate any one of the properties--volume, pressure, temperature, or moles of gas present-- given the other three. A gas that obeys this equation is said to behave ideally.
http://www.youtube.com/watch?v=wVVjaJmMWoQ
From the ideal gas equation we can derive the combined gas law, P1V1 / T1 = P2V2 / T2 which holds when the amount of gas (moles) remains constant.
The pressure of a gas mixture is described by Dalton's law of partial pressures, which states that the total pressure of the mixture of gases in a container is the sum of the partial pressures of the gases that make up the mixture.
The kinetic molecular theory of gases is a model that accounts for ideal gas behavior.
What is STP?: http://chemistry.about.com/od/gas2/f/What-Is-Stp-In-Chemistry.htm
You have 1.05 grams of KlO2, how many moles will form of O2? {Answer: 0.289 LO2}
http://www.youtube.com/user/EducatorVids?v=jykTDKZQ9eo&feature=pyv&ad=8587456388&kw=chemistry
http://www.glenoaks.edu/facultystaff/FacultyWebSites/SarahSimmons/Documents/NSC-130%20Stoichiometry%20Worksheet.pdf
Liquids: have a definite volume but assumes the shape of the container
Gases: have no definite shape
Liquids and gases are considered fluids
Boyle’s Law: states that the volume of a given amount of gas is inversely proportional to its pressure (at constant temperature): PV=k or P=k/V. As pressure increases, volume decreases.
http://www.iun.edu/~cpanhd/C101webnotes/gases/boyleslaw.html
Atmospheric pressure
- measured with a barometer
- the most commonly used units of pressure are mm Hg (torr), atmospheres, and pascals (the SI unit).
Charle's law
- For a given amount of gas at constant pressure, the volume is directly proportional to the temperature (in kelvins): V=bT.
- For a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas: V=an.
These three laws can be combined into the ideal gas law, PV=nRT, where R is called the universal gas constant.
This equation makes it possible to calculate any one of the properties--volume, pressure, temperature, or moles of gas present-- given the other three. A gas that obeys this equation is said to behave ideally.
http://www.youtube.com/watch?v=wVVjaJmMWoQ
From the ideal gas equation we can derive the combined gas law, P1V1 / T1 = P2V2 / T2 which holds when the amount of gas (moles) remains constant.
The pressure of a gas mixture is described by Dalton's law of partial pressures, which states that the total pressure of the mixture of gases in a container is the sum of the partial pressures of the gases that make up the mixture.
The kinetic molecular theory of gases is a model that accounts for ideal gas behavior.
What is STP?: http://chemistry.about.com/od/gas2/f/What-Is-Stp-In-Chemistry.htm
You have 1.05 grams of KlO2, how many moles will form of O2? {Answer: 0.289 LO2}
http://www.youtube.com/user/EducatorVids?v=jykTDKZQ9eo&feature=pyv&ad=8587456388&kw=chemistry
http://www.glenoaks.edu/facultystaff/FacultyWebSites/SarahSimmons/Documents/NSC-130%20Stoichiometry%20Worksheet.pdf