GL - Gas Laws (Module Overview)
Gas Laws
Introduction
Recall from previous modules that matter can take the form of various phases; solid, liquid, gas and sometimes plasma. In this module, we will investigate the properties of gases. We will take a look at the Kinetic Molecular Theory as a basis for explaining the behavior of gases, and solve common gas law equations.
Having a periodic table handy is always helpful in chemistry. You may always use a periodic table on assignments, quizzes, and tests in this course. Feel free to download the periodic table below:
Download the periodic table. Links to an external site.
In addition to the periodic table, this module presents many gas laws. Although you are required to know when and how to use each equation, you are not required to have the equations memorized. Use the formula sheet below as a reference when completing gas law calculations. You may use it on all assignments, quizzes and the module test.
Download the Gas Laws Formula Sheet. Links to an external site.
Module Lessons Preview
In this module, we will study the following topics:
Kinetic Molecular Theory: In this lesson, we will see how balloons and marshmallows can be used to discuss the various properties of gases and the components of the Kinetic Molecular Theory.
Ideal Gas Law: Students will have the opportunity to investigate air bags to simulate the properties of an ideal gas.
Molar Volumes of Gases: We will revisit some stoichiometry concepts to learn about one additional conversion factor used to convert between moles and volumes of gases.
Gas Laws Calculations: In this final lesson, we investigate the relationship between the pressure, volume and temperature of gases.
Key Terms
kinetic theory - physical theory that explains the behavior of gases on the basis of the following assumptions: (1) Any gas is composed of a very large number of very tiny particles called molecules; (2) The molecules are very far apart compared to their sizes, so that they can be considered as points; (3) The molecules exert no forces on one another except during rare collisions, and these collisions are perfectly elastic, i.e., they take place within a negligible span of time and in accordance with the laws of mechanics.
ideal gas - A gas that, when kept at a constant temperature, would obey the gas laws exactly. No known gas is an ideal gas.
pressure - Force applied uniformly over a surface, measured as force per unit of area.
atmosphere - A unit of pressure equal to the air pressure at sea level. It equals the amount of pressure that will support a column of mercury 760 millimeters high at 0 degrees Celsius under standard gravity,
kilopascal - One thousand (103) pascals; the metric unit of pressure; one pound per square inch is equal to 6.89 kilopascals; abbreviated kPa.
mm Hg - A unit of pressure that is equal to approximately 1.316 × 10 - 3 atmospheres or 133.3 pascals.
atmospheric pressure - Pressure caused by the weight of the atmosphere. At sea level it has a mean value of one atmosphere but reduces with increasing altitude.
standard temperature - A temperature of 0°C or 273 Kelvin.
standard pressure - A pressure of 1 atmosphere (101,325 newtons per square meter), to which measurements of quantities dependent on pressure, such as the volume of a gas, are often referred.
STP - standard temperature and pressure
barometer - An absolute pressure gage specifically designed to measure atmospheric pressure. This instrument is a type of manometer with one leg at zero pressure absolute.
manometer - A double-leg liquid-column gage used to measure the difference between two fluid pressures.
Boyle's Law - The principle that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure. P1V1=P2V2
Charles' Law - The physical law that the volume of a fixed mass of gas held at a constant pressure varies directly with the absolute temperature.V1/T1=V2/T2
Gay-Lussac’s Law - When volume is held constant, the pressure and temperature of a gas are directly proportional. P1/T1 = P2/T2
Ideal Gas Law - The equation of state of an ideal gas which is a good approximation to real gases at sufficiently high temperatures and low pressures; that is, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, T is the temperature, and R is the gas constant.
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