Chemistry and Chemical Reactivity Essay

The Kinetic Molecular Theory of Gases (KMT) is an explanation and description of the motion and behavior of molecules. It looks into the kinematics of molecules, wherein centering on the forces exists in the midst of molecules and the energy generated by the motion of these molecules (Poseidon Softw be and Invention, 1997). Etymologically, the KMT comes from energising which means moving, and molecular which comes from the group word molecule, classically the smallest unit of particle.The KMT includes several postulates which describe how the molecules of fuck upes behave. The following are characteristics of how gas molecules behave (1) Gases are composed of very small particles called molecules (2) the molecules are very large in number (3) they are suddenly spherical in shape and elastic in nature (4) their volume is negligible which implies that they can give notice freely (Dogra, 1984) (4) the average distance between molecules is relatively large as compared to their s ize (Kotz, et al. , 2008) (5) they behave in a state of continual, random motion following Newtons faithfulnesss (Selvaratnam, 1998) (6) they move in a straight line until they collide with another particle or with the walls of the container (Whitley, 2005, n. p. ).(7) the collisions of the gas molecules with other particles or with the walls of the container are suddenly elastic such that the total energising energy after the collision is equal to the total kinetic energy before the collision (8) there are no attractive or repulsive forces between the molecules, and only during collisions do the particles exert forces on each other (Wulfsberg, 2000) (9) there is no energy disjointed during the collisions energy is conserved and (10) the average kinetic energy of the particles depends on the temperature of the system.These postulates can be further illustrated in terms of the interpretation of the temperature and pressure of a gas. Temperature, being a macroscopic characteristi c of matter, is interpreted in terms of the kinetic energy of the molecules (Selvaratnam, 1998, p. 183). There is a directly proportional relationship between the temperature and the kinetic energy of the molecules of a gas. This means that an increase in temperature becomes a similar increase in the kinetic energy or rapid movement of the molecules.The hotter the gas is, the faster its particles move (Whitley, 2005, n. p. ). Pressure, on the other hand, is due(p) to the incessant bombardment of the walls of the container vessel by the billions and billions of molecules present (Selvaratnam, 1998, p. 183). This only means that if more collisions occur, the pressure is higher. The idiosyncratic gas laws could be put into perspective in relation to the KMT. According to Boyles Law, at constant number of moles and temperature, pressure and volume are inversely proportional (Whitley, 2005, n. p. ).Charles Law, on the other hand, states that at constant number of moles and pressure, t he volume and the temperature are directly proportional (Whitley, 2005, n. p. ). A third Gas Law consists of the theory that at constant number of moles and pressure, the volume and the temperature are directly proportional (Whitley, 2005, n. p. ). These individual gas laws, if combined, would produce an ideal gas. In relation to the motion of the molecules, the molecular activities in the three states of matter disaccord in several aspects.In the solid state, the particles are packed in a more nearly manner. They are held closely to one another by their attractive forces (Poseidon Software and Invention, 1997). These strong, attractive forces between the particles cause them not to move freely and instead, vibrate. This feature results in a definite shape and volume of solids. In the liquid state, the intermolecular forces only permit the particles to flow or glide over one another. As compared to solid, the motion of the molecules is more random.The shape and volume of a liquid is dependent on its container. The intermolecular forces are also essential in understanding the dissolution of things. In the dissolving process, the molecules of the solute are surrounded by the molecules of the solvent. Here, molecular bonds between molecules of solute have to be broken and molecular bonds of the solvent also have to be disrupted (Educating Online, 2007, n. p. ).ReferencesBlauch, D. N. (2001). Kinetic Molecular Theory. Retrieved March 6, 2009 from http//www. chm. davidson. edu/chemistryapplets/kineticmoleculartheory/BasicConcepts. html. Dogra, S. (1984). Physical Chemistry through Problems. India New Age International. Educating Online. (2007). solvability of things. Retrieved March 6, 2009 fromhttp//www. solubilityofthings. com/basics/why_things_dissolve. php Kotz, J. C. , Treichel, P. & Weaver. (2008).Chemistry and Chemical Reactivity. U. S. Cengage Learning EMEA Poseidon Software and Invention. (1997, November 16). Kinetic Molecular Theory. Retrieved March 6, 2009 from http//www.psinvention. com/kinetic. htm. Selvaratnam, M. (1998). A Guided Approach to Learning Chemistry. South Africa Juta and Company Limited. The Kinetic Molecular Theory. (2009). Bodner Research Web. Retrieved March 6, 2009 from http//chemed. chem. purdue. edu/genchem/topicreview/bp/ch4/kinetic4. html. Whitley, K. (2005, may 13). Kinetic Molecular Theory of Gases. Retrieved March 6, 2009 from http//www. chemprofessor. com/kmt. htm. Wulfsberg, G. (2000). Inorganic Chemistry. U. S. University Science Books.