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1. State the five assumptions of the Kinetic-Molecular Theory of gases. a) Gases consist of large numbers of tiny particles. These particles, usually molecules or atoms, typically occupy a volume about 1000 times larger than occupied by the same number of particles in the liquid or solid state. Thus molecules of gases are much further apart than those of liquids or solids.
Most of the volume occupied by a gas is empty space. This accounts for the lower density of gases compared to liquids and solids, and the fact that gases are easily compressible. b) The particles of a gas are in constant motion, moving rapidly in straight lines in all directions, and thus passes kinetic energy. The kinetic energy of particles overcomes the attractive forces between them except near the temperature at which the gas condenses and becomes a liquid. Gas particles travel in random directions at high speeds. c) The collisions between particles of a gas and between particles and container walls are elastic collisions.
An elastic collision is one in which there is no net loss of kinetic energy. Kinetic energy is transferred between two particles during collisions, but the total kinetic energy of the two particles remains the same, at constant temperature and volume. d) There are no forces of attraction or repulsion between the particles of a gas. You can think of ideal gas molecules as behaving like small billiard balls.
They move very fast, and when they collide they do not stick together, but immediately bounce apart. e) The average kinetic energy of the particles of a gas is directly proportional to the Kelvin temperature of the gas. The kinetic energy of a particle (or any other moving object) is given by the equation: KE = 1 / 2 mv 2. Where m is the mass of the particle and v is the velocity. 2. List the five properties of gases (add the extra one too! ) a) Expansion Gases do not have a definite shape of definite volume. They fill the entire volume of an container in which they are enclosed and assume its shape.
A gas transferred from 1 -L to a 2 -L vessel will quickly expand to fill the entire 2 -L volume. b) Fluidity Because the attractive forces between gas particles are negligible, gas particles glide easily past one another. This ability to flow causes gases to show mechanical behavior similar to that of liquids. Because liquids and gases flow, they are referred to collectively as fluids. c) Low density The density of a substance in the gaseous state is about 1 / 1000 the density of the same substance in the liquid or solid state because the particles are so much farther apart in the gaseous state. For example, oxygen gas has a density of. 001 g / m L, at 0 C and 1 atmosphere pressure.
As liquid at - 183 C, oxygen has a density of 1. 149 g / m L. d) Compressibility During the compression of a gas, the gas particles which are initially very far apart, are crowded closer together. Under sufficient compression, the volume of a given sample of gas can be decreased thousands of times. The steel cylinders containing nitrogen, oxygen, or other gases under pressure that are widely used in industry illustrate this point. Such cylinders have internal volume of about 55 L. When they returned "empty" at ordinary pressures, they contain about 55 L of gas, although when they were delivered "full" they may have had 100 times as many molecules of gas compressed within the same cylinder.
e) Diffusion Gases spread out and mix with one another without stirring and in the absence of circulating currents. If the stopper is removed from a container of ammonia, the presence of this gas, which irritates the eyes, nose, and throat, soon becomes evident. Eventually, the ammonia mixes uniformly with the air in the room, as the random and continuous motion of the ammonia molecules carries them throughout the available space. The spontaneous mixing of the particles of two substances because of their random motion is referred to as diffusion. f) Exertion Gases also have the ability to exert pressure on a surface. 3. Methods of production of the representative gases. 1) Balanced equations required: a) Oxygen (2 methods): One method of preparation is decomposing hydrogen peroxide.
Oxygen can be prepared by passing hydrogen peroxide through a catalyst, manganese dioxide. It is then collected by water displacement. The second method is decomposing water through electrolysis. Electricity is passes though water, separating Hydrogen and Oxygen. Method 1: 2 H 2 O 2 (aq) -MnO 2 2 H 2 O (l) + O 2 (g).
Method 2: 2 H 2 O (l) -electrical energy 2 H 2 (g) + O 2 (g). b) Ozone (1 method): If enough energy is present, O 2 will become O 3. Method: 3 O 2 (g) + energy 2 O 3 (g). c) Hydrogen (2 methods): One of the methods of preparing Hydrogen is just like preparing Oxygen, through the use of electrolysis. Method 1: Method 2: 2 H 2 O (l) -electrical energy 2 H 2 (g) + O 2 (g). Another commonly used method is reacting metals with acids.
Method 2: Zn (s) + H 2 SO 4 (aq) Zn SO 4 (aq) + H 2 (g). d) Ammonia (1 method): The Haber Process is the catalytic synthesis of ammonia from nitrogen gas and hydrogen gas. Method: N 2 (g) + 3 H 2 (g) catalyst 2 NH 3 (g). 2) Description of method required: a) Carbon Dioxide: Carbon dioxide is usually produced when combustion of carbon compounds occur, decompose carbonates, and aerobic respiration. b) Carbon Monoxide: Carbon Monoxide is commonly produced when incomplete combustion occurs. Most carbon monoxide comes from the exhaust of cars.
c) Nitrogen: In laboratories, Nitrogen is produced by heating certain compounds that contain ammonia. 4. List the physical and chemical properties of gases in SQ 8. Oxygen: Physical - Oxygen is a gas that is odorless, colorless, tasteless, and is denser than air. It appears to be a pale blue color when in liquid and solid states. Chemical - Very electronegative and tends to form oxides and peroxides. Ozone: Physical - Ozone is a gas that is pungent, pale blue in color, and tastes bitter.
Its Lewis Dot structure is resonance. Nitrogen: Physical - Nitrogen is a gas that is odorless, colorless, tasteless, and less dense than air. The liquid states is commonly used for freezing involving medical purposes. It appears white in its solid form. Chemical - Because of its triple bond, nitrogen is not very reactive. It tends to react with hydrocarbons to form photochemical smog.
Ammonia: Physical - Ammonia is a gas that is strong and pungent, it is colorless, and tastes bitter. Carbon Dioxide: Physical - Carbon Dioxide is a gas that is distinct in scent, colorless, and tastes sour. It s denser than air and its Lewis Structure is resonance. Chemical - Extremely stable, absolutely does not support combustion. Carbon Monoxide: Physical/Chemical - Carbon Monoxide is a gas that is very toxic and almost impossible to tell if it is present. Hemoglobin is also 300 times more susceptible to Carbon Monoxide than Oxygen.
Hydrogen: Physical - Hydrogen is a gas that is odorless, colorless, tasteless, and less dense than air. It is clear in both liquid and solid states, it appears to be ice-like in its solid state. Chemical - Hydrogen is highly reactive. It basically rates with anything around it. Mostly in existance with compounds involving non-metals. 5.
Know some of the uses of the gases in SQ 8. Oxygen: Commonly used in aerobic respiration and combustion. Nitrogen: Commonly used to freeze things for medical purposes, cooling, and propellant for aerosol products, also used to prolong life of food products. Carbon Dioxide: Commonly used in baking to make dough rise, used for freezing, plants use it for producing glucose, and fire extinguishers.
Hydrogen: Commonly used for hydrogenation and fuel. 6. A colorless, odorless and tasteless gas is found. What are some of the tests and results which can be used to identify the gas? Which gases can be eliminated based on odor? Color?
Which gas is most difficult to identify? Possibilities for colorless odorless and tasteless gas: Oxygen, Nitrogen, Carbon Monoxide, and Hydrogen. If Oxygen was in a test tube and you placed a bring splint up to it, it should suck the flame in and make a "pop" sound. Or it would re-ignite a glowing splint.
o Only Oxygen and Ozone have color in their liquid and solid states. o Only Carbon Dioxide, Ozone, and Ammonia have odor. The most difficult gas to identify would be Hydrogen. 7. Define allotrope Allotrope - One of the two or more forms of an element that exists in the same physical state. 8. What is a eudiometer?
Eudiometer - A eudiometer is a gas collecting tube. 9. What kinds of attractive forces exists between molecules? Describe all three. How are these attractive forces different from those we studies previously? Intermolecular forces - The forces of attraction between molecules. Dipole-dipole forces - The forces of attraction between polar molecules.
London dispersion forces - Intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles and induced dipoles. 10. What is an ideal gas? When does a real gas behave like an ideal gas? An ideal gas is a gas that fits the kinetic molecular theory perfectly. Noble gases tend to behave like an ideal gas.
Real gases behave like an ideal gas when it fits the 5 assumptions of KMT.
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