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Describing Gases.pptx...................
- 2. Every matter has its own properties. Matter has three states that differ from each other. Their differences in their properties are based on the arrangement of their particles. Under normal atmospheric condition, there are only 11 elements that are gases (diatomic molecules hydrogen, nitrogen, oxygen, fluorine, and chlorine and the noble gases helium, neon, argon, krypton, xenon, and radon. Ozone, another form of oxygen, is also a gas at room temperature.
- 3. Volume • Molecules of gases occupy a space. It may be proven when the gas fills up its container . • 1 L = 10 dm = 10 m = 1000 mL = 1000 cm • Its SI is in liters (L). It can also be expressed in milliliters (mL), cubic centimeters, Pressure Temperature Amount of gas 3 3 3 3 • The physical force exerted on an object. Pressure of the gas is the force exerted by the gas per unit area. • Pressure(P) = Force (F) / Area (A) • 1 atm = 760 mm of Hg = 760 torr = 1.01325 bar = 101.325 kPa • The SI unit used for • The temperature of a gas depends on the kinetic energy of the gas. Gases expand when temperature is increased. • K= C + 273.15 • The temperature of the gas is generally expressed in Fahrenheit, • The mass of the gas is related to the number of moles of the gas. • number of moles (n) = mass of the gas / molar mass of the gas • The mass of the gas is generally expressed in kilograms (kg) or grams (g) Fundamental Properties of Gas
- 4. • The behavior of gases is determined by the behavior of its individual particles. • The kinetic molecular theory was formulated using a simple model. • In 1870, scientist were able to make a model of ideal gas or theoretical gas. • The particles of an ideal gas behave consistently and in a predictable manner. • It serves as a basis which attempts to explain the behavior of real gases. Kinetic Molecular Theory
- 5. Characteristics of Gas Gases like any other states of matter, consists of very tiny particles, each of which has mass. The density of gases varies with changes in temperature and pressure. Gases are most likely empty space because of a wide distance between these tiny particles. Thus, making gases compressible and have low density.
- 6. Characteristics of Gas Gas particles move rapidly in straight lines, travel constantly and in random directions. Because of the wide spaces between gas particles, the forces of attraction (Van der Waals Force) between them are negligible. Gases diffuse very rapidly that allows two or more gases to mix readily when combined.
- 7. Characteristics of Gas Gas particles collide with each other or with the walls of its container but do not lose their kinetic energy; instead, it is only transferred to the lower- energy particle and will continue to move. In short, energy is conserved in All gases have the same average kinetic energy at a given temperature of gas. The average kinetic energy of gas particles is directly proportional to the absolute temperature of the gas. this means that gas particles may have higher kinetic energy at a higher
- 8. THE GAS LAWS
- 9. The four measurable properties of gases such as pressure, volume, temperature, and number of moles are related to each other. There are four main gas laws. These are Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, and Avogadro’s Law. These laws are products of various experiments that are done many centuries ago. The Ideal Gas Law can be used to describe the relationship between variables used by the four main gas laws.
- 10. • Proposed by Robert Boyle, an Anglo-Irish chemist. • He investigate the relationship between pressure and volume of a gas using a J- shaped tube apparatus. • He proposed that the volume of a given mass of gas held at constant temperature is inversely proportional to its pressure. • Boyle shown that as the volume decreases, the pressure increases. BOYLE’S LAW