applications of kinetic molecular theory to solids and liquids?
817765
kinetic just means movement. So it is like how molecules vibrate. The more they vibrate the further apart they get and more energy they have. So a solid can have molecules vibrating slower but add more heat it can turn to a liquid.
1058187
for a rigid rotor, the transition lines are equally spaced in the wavenumber space. However, this is not always the case, except for the rigid rotor model. \n\nfor non-rigid rotor model, we need to consider changes in the moment of inertia of the molecule due to centrifugal distortion and the effects of vibration on the rotation.\n\nthe formulas are hard to write here, better to look at the references in \nhttp://en.wikipedia.org/wiki/Rotational_spectroscopy\nor elsewhere.
95223
forcing water away because they are polar molecules
1143670
(m)\n\nFor many years scientists have tried to understand the unique properties of ice in terms of the behavior of the molecules in the topmost layer. However, despite extensive studies the exact structure and dynamical motion of the individual water molecules at the ice surface have remained elusive. An international team of physicists (J. Braun, A. Glebov, A. P. Graham, A. Menzel) in the group of Peter Toennies at the Max Planck Institute for Fluid Dynamics in Göttingen have used the scattering of very low-energy He atoms for the successful analysis of the structural arrangement of water molecules on the ice surface and have also gained direct information on their vibrational motion. The results of these experiments, published in the March 23 issue of the Physical Review Letters [80, 2638 (1998)], indicate that the molecules are surprisingly mobile which explains many peculiarities in the interactions of ice with its environment. \n\nWhy do solid ice crystals have a melted surface-layer at temperatures far below the bulk melting point 0°C, that allows us to ski, skate and slide so easily; Why do two pieces of ice, when put together, adhere and become one; Why are different molecules in the earth stratosphere easily trapped on the surface of ice particles, where they can react, with consequences such as depletion of the ozone layer? This wide variety of intriguing questions have made ice one of the most frequently studied materials. However, until now, no definite answers to these and many other questions have been forthcoming since all of the attempts to gain information on the microscopic structure of a single crystal ice surface have failed. Very recently, even the powerful method of electron diffraction, routinely used in surface structure analysis, failed to provide any clear evidence on the structural arrangement of the topmost layer of ice. The group of scientists from the Lawrence Berkeley National Laboratory, Free University in Amsterdam, and the University of Pierre and Marie Curie in Paris [Surface Science 381, 190 (1997); also see report of Charles Seife in Science 274, 2012 (1996)] have suggested, on the basis of theoretical simulations, that the uppermost water molecules vibrate so strongly that a coherent diffraction pattern cannot be observed.\n\nIn the attempt to resolve this problem the researchers in Göttingen have employed low-energy helium atom scattering. This technique has the advantage of being completely nondestructive and exclusively sensitive to the topmost layer of crystals. Since the (111) surface of platinum has nearly the same lattice spacing as ice, it was used as a template on which single crystal ice films of 10-100 nm thickness were grown. Only after cooling the surface to 30 K was it possible to observe a sharp intense series of diffraction peaks. These not only provide information on the lattice spacing and arrangement of the first layer molecules but also indicate at least a partial alignment of the hydrogen atoms (ferroelectric ordering) at the surface.\n\nA further advantage of the He atom scattering technique is that with the same equipment high-resolution time-of-flight energy loss and gain spectra can be measured. These spectra provide information on the frequencies and wave-lengths of the collective vibrations (phonons) at the surface. As the crystal was again cooled down to 30 K, a very intense inelastic peak emerged from a strong multiphonon background. This intense inelastic peak was simulated with a theoretical model which allowed its assignment to a special very large amplitude in-plane shearing motion of the surface molecules. At higher temperatures, this motion becomes increasingly enhanced leading to a high density "phonon bath" and ultimately individual molecules will break away from their original sites. This explains the liquid-like topmost layer as well as the difficulties experienced in the electron diffraction experiments.
981009
1. melting point\n2. expand to occupy the entire volume of the closed container\n3. thermal energy is a measure of the average kinetic energy of the particles also known as temperature.\n4. sorry - I don't get the question
174163
thermodynamics?  heat transfer?  physics?
512153
The mean van der Waals diameter of water has been reported as identical with that of isoelectronic neon (2.82 Å) [112]. Molecular model values and intermediate peak radial distribution data indicates however that it is somewhat greater (~3.2Å). The molecule is clearly not spherical, however, with about a ±5% variation in van der Waals diameter dependent on the axis chosen; approximately tetrahedrally placed slight indentations being apparent opposite the (putative) electron pairs.
699724
fluids - convection is due to the movement of molecules
749646
Try doing a Google search under the Hall or the Hall-Heroult process.    That or check out a General or an Inorganic Chemistry book from the library.  That's a good launch point.
687306
Check the Michaelis-Menten equation.It's too long to write it all down for you ;)
94512
A ContinuumModel for the Transition Regime:\nSolutions of Instationary Problems\nby the Moment Method URL: \n\nhttp://www.math.princeton.edu/~mtorrilh/Publications/Torrilhon_RGD2002.pdf\n\n\nExperimental Investigation and Mathematical Simulation\nof the Ignition of Methane/Air Mixtures URL:\n\nhttp://www.cheng.cam.ac.uk/research/groups/laser/Publications/Clemens/paper_14.pdf\n\nI hope these help....\n\nDon
202441
The physical science and technology of the static and dynamic behavior of fluids.
569322
Use the ideal gas law \n\nPV/T = constant for the final and initial states.
1055255
the diffusion of liquids and gasses are limited by the cohesive bonds between the composite molecules, and en masse by the forces of gravity in the y axis and friction and cohesion in the x-z plane.  In a gas, the inter-bonding is limited or nil, so each molecule has more degrees of freedom and hence more statistical probability of random scattering, or diffusion.
1021437
a) \n\nThe molecules in a substance are in constant motion. Now there are two oppposing forces on a substance. One is the intermolecular bond energy that tries to keep the molecules together. The other is the kinetic energy of the molecules that tries to push the molecules apart (these two forces work together to keep substances in equilibrium - basically keeps it from exploding or imploding in simple terms).\n\nNow, in solids, the molecules have low kinetic energy but high intermolecular bond energy(IBE). Liquids, the kinetic energy is higher and conversely the IBE is lower. Gases, the kinetic energy is high and the IBE is low (makes sense - the "bond" is weak)\n\nSo now, the kinetic energy or molecules is directly proportional to the heat applied - the hotter it is, the more kinetic energy the molecules have. Therefore when you heat it ... the kintic energy gets stronger and stronger and the IBE gets weaker and weaker until it breaks and the substance undergoes its change of state.\n\nHope this explained it well!
1089808
Grab your textbook or go to wikipedia.\n\nSee:\n\n1. Random Molecular Motion\n2. Diffusion\n\nThe simple answer is that atoms and molecules move constantly because they have energy, the amount of energy something has can be measured, in your example through heat. The less energy something has, the slower it will move and conversely the more energy something has the faster it will move. This is random molecular motion.\n\nDiffusion is the motion of these molecules from areas of abundance to areas scarcity. Molecules will diffuse until they are evenly distributed throughout a solution. Too illustrate this try to think of the molecules as marbles in a box, in the beginning they are all bunched up in one corner, but if you start to shake the box they will begin to bump against one another, at first rapidly because they are all bunched up. As time goes on they will spread out until they fill the entire box and are bumping up against each other at a rate that keeps them as evenly spread out as the box allows. The amount of energy you apply to the shaking will cause them to move faster or slower, or in your example, cold water will make the food coloring distribute slower and hot water will make them distribute faster.
282222
Well, enzymes ARE catalysts, at least to my knowledge.\n\nThere isn't sufficient information to describe the collision rate. In Kinetics, we determine the collision rate using the rate equation, and that is determined using the R.D.S. (rate determining step) or slow step of the mechanism of the reaction... and since you have none of these in your question, it's really quite impossible to answer!