what is happen in molecol while expansion a solid?
955519
The density of a solid or liquid is determined by the various kinds of intermolecular bonds, see the reference.  These bonds tend to attract a molecule to its neighbors.  The molecules tend to keep getting closer until the electrostatic repulsion between the positively charged nuclei equals the attraction.\n\nAs you increase the temperature, nothing changes within a molecule, the molecules just move more.  In a solid, they generally stay in place and vibrate with respect to their neighbors.  The repulsive force is inverse square with distance, so as molecules get closer, the repulsive force increases rapidly.  Thus, the vibrations involve more movement away from the neighbors than toward the neighbors.  That's why the average distance between molecules increases with temperature.\n\nRarely, other factors dominate.  As water cools, it contracts until it reaches about 39 degrees F, and then starts expanding.
538394
This is a purely physical change of state from solid to liquid as a result of energy being added to the system.  There is an increase in entropy of the system.
679263
I think that what is troubling you could be an exerecise involving "molarity" which uses two quantities: mass(moles)/volume(liter). \nBut you have to bear in mind that mass is referred to the solute, and volume refers to the solution. So, these quantities are not referring to ONE substance. \nIt would be better if you posted a question with the whole exercise, for clarity. \nGood luck.
30902
That last answer is slightly confused. By Charle's law (called Gay-Lussac's Law in France), V1/T1=V2/T2 at constant pressure, where Vs are volume and Ts are temperature. Therefore, if one increases the temperature T1 >T2, then one would expect the volume to increase as well, so V1>V2. \n\nHowever, this is assuming equal pressure. Obviously, as the temperature of the balloon increases, one might expect the pressure to increase as well. This situation is governed by the universal gas law, PV=nRT, and as temperature T increases, one would expect the product PV to increase as well, probably some increase in pressure P and some increase in volume V, depending on how stretchy the balloon is. Another factor that comes into play is that balloons are permeable, so as the pressure increases, more gas inside the balloon will diffuse out of the balloon, decreasing the volume of the balloon. \n\nI would expect that over a short period, the balloon would expand from the heating of the gas inside, but over a longer period, the heat and pressure would encourage enhanced diffusion, causing the ballooon to shrink. \n\nIn cold water, obviously diffusion will not operate as efficiently, and one will have a more straightforward application of the universal gas law, so that the product PV will decrease with decreasing temperature over both the short and long terms. \n\nThe rate at which the heated balloon contracts due to loss of air inside by diffusion depends on the permeability of the balloon surface.
32393
No, a subliminating substance goes from a solid directly to a gas.  If you heat wax, it turns into a liquid.
334077
You need to give more information about the shape to get a definitive answer.  If the cell were cubical, then the volume increases 1000 times if all three sides increase 10 times in length.
446916
It differs depending on whether you are speaking of parallell or perpendicular to the surface\nand\nat what temperature it is\n\n8 > 36(10-^6/K)   {@ 0 - 1000°C}\n\nparallel and lower temperatures = lower CTE\n\nCoefficient of expansion per °C parallel to cleavage:\n  0° > 200° C *  8x10^-6 >  9x10^-6\n200° > 500° C * 10x10^-6 > 12x10^-6 \n\nCoefficient of expansion per °C perpendicular to cleavage:   \n 20° > 100° C * 15x10^-6 > 25x10^-6\n100° > 300° C * 15x10^-6 > 25x10^-6\n300° > 600° C * 16x10^-6 > 36x10^-6
795464
wow... opposite answers to the same question... hmmm In a sense, they are both correct. The volumetric changes experienced by solids due to temperature changes is very small, but there is a slight change indeed. Every solid has its own coefficient of volumetric change for every degree change in temperature. A prime example of solids changing volume are the expansion joints you see in bridges. Also, I think the empire state building is like 6 inches taller in summer than in winter... something like that. Gasses on the other hand experience much larger volumetric changes. Temperature as well as pressure will greatly affect the volume of a gas. Consider oxygen, it can be compressed to a liquid. \n\nOn the other hand, let me second guess this question, maybe it should read, why can a gas be compressed and not a liquid? In a gas, the molecules are spaced wide apart, farther apart than their electric charges do not affect the molecule next to them. In a liquid, the molecules are packed as tight as they physically can be packed. They cannot be compressed farther. Only temperature can affect the volume of a liquid as mentioned above. Hope this helps some!
943587
It's not expanding: cell contents will overlap the following cells if they are empty. Just type a space in the cell to the right of your data and it will stop overlapping.
895484
SURFACE AREA INCREASES\n\nIT'S VICE VERSA
152571
By heating the lid is bigger than it was, and bigger than the jar. So the lid is just seems like other bigger jar's.\nEven if you heated the metal lid and the gas together, you will get the same result, as jar's expansion is less than the lid's expansion.
50274
Chemical equations show the molecular composition of compounds in a balaanced form between reactants and products. These are expressed in moles, or number of molecules, rather than mass. By matching the number of molecules needed for a reaction the result can be controlled better than if only mass were used. Excess or limited amounts of one element in a reaction might cause the product to be different than intended. Ultimately, a chemical engineer will convert the specifications to mass, but unless the molarity of the raw material is known this cannot be done properly.
362520
P, expanded octets dont happen to atoms in the first or second rows.
309381
D.liquid to gas\nwhen the molecules move with increased speed, their average kinetic energy increases, causing the intermolucular forces to weaken and so they move further away from each other and eventually change phase. this is exactly what happens when you heat something, the molecules, gain energy, vibrate about theuir mean positions, at thresh-hold amplitudes or velocities, they break the molecular forces and chenge phase from solid to liquid or liquid to gas
1142195
Since this the "Chemistry" section. Let's answer this with Chemistry.\n\nIf you're superhot this means that you're in gaseous phase. As a gas you will expand until you occupy the whole volume of the room where you are with the horny gal. since you are changing you volume and considering that the T of the room and your mass remain constant during the expansion, then you can use the ideal gas equation to establish what happen in the room.\npV=nRT, since n,R, and T are constant in this problem, we can write:\n\np1*V1=p2*V2\nto calculate the new pressure in the room (p2):\n\np2=(p1*V1)/V2\n\nsince the final volume in bigger than the initial, this equation establishes that the pressure in the room will be lower that the original one (before you get gaseous).\nThe suddenly change in pressure will cause an implotion (opposite to explotion) crashing your horny gal in the room.
1037023
Water, when heated from a solid to liquid state, but ultimately in a gaseous state it again expands.  It still obeys all the laws of chemistry, but the bonds just arrange themselves in a more space efficient manner in liquid than in solid form.\n\nAnd moses with a P, no metals exist with the properties you say.  It is physically impossible, sorry man, but I'm a biochem major and it's my job to know what stuff does under different stresses, and nothing does what you claim.  However, if you do have a material that does this, get in touch with me, we'll talk to the patent office, and we'll license it out to companies for billions of dollars.
950681
Van derWaal's equation is this:\n(P+a(n/V)^2)(V-nb)=nRT\n\nThe ideal gas law is:\nPV=nRT\n\na) b will lower the total volume, accounting for the space taken up by the molecules.  True.\n\nb) a will increase the volume based on intermolecular repulsive forces.  True.\n\nc) The attraction will decrease the pressure.  False.\n\nd) The individual particles will stay a constant size; the volume and pressure don't change bond lengths or shell sizes, just the spacing between the particles.  True.