what is the ideal gas principle?
609601
Ideal Gas Law:\n\nPV=nRT\n\nwhere P - pressure, V - volume, n - no. of moles, R - Universal Gas Constant, T - temperature (in K)
978427
you mean What are physical science principles?\nwww.ask.com
739100
I can't answer the question, but you need Boyle's Law, the volume of a gas is inversely proportional to it's pressure.  Also, are you assuming there is no temperature change?
826041
The answer to your question would depend on (1) whether "empty" means a "perfect vacuum" or filled with air? (2) how is this 1 joule of energy initially distributed inside this box? (3) how large is this box? (4) how much time is allowed to elapse before the termperature is determined? (5) can energy leak out or into the box? (6) is the box under the influence of a gravitational field?\n\nThe temperature of an object is proportional to the average kinetic energy of the molecules in it. In a pure vacuum, there are no molecules. There is nothing to measure the kinetic energy of, and temperature is undefined. If a thermometer were placed in a vacuum, the reading would be a measurement of the internal temperature of the thermometer, not of the vacuum which surrounds it. So having 1 joule of energy inside a box containing pure vacuum would have NO temperature. And if it contained air, then we would need to know the initial temperature, pressure of the air inside the box and also the volume of the box. Then we can approximate the air as an ideal gas and use the following equation to compute the temperature:\n\nPV=nRT\n\nwhere T is the temperature, n is the number of moles of gas and R is the gas constant. Since we know the initial temperture and pressure, and the volume of the box. Then\n\nP(i)V(i)/T(i) = P(f)V(f)/T(f)\n\nT(f) = T(i) [P(f)/P(i)]\n\nSince pressure is dfined as P = F/A (force per unit area) and\n\nE = Fd (force times distance), then\n\nP = E/Ad, where Ad = V volume of the box (here we are assuming that the 1 joule of energy is uniformly distributed inside the box and the volume of the box does not change)\n\nHence, T(f) = T(i) [E/P(i)V(i)]
129942
the ideal gas law is:\n \n PV = nRT \n\nSO,\n\n P= .95 atm\n n=  .87\n T=  280K\n R=  .0821\n V=  ?\n\n solve for V\n\n     V = nRT/P =(.87* .0821* 280) /.95 = 21 liters
193517
You don't provide enough data to determine this.  The gas law PV=nRT has variables you need to define.
112298
Ideal gas laws assume that all particles are spherically symmtric and engage only in elastic collisions.  They ignore all other types of molecular energy (rotation in other planes of symmetry or asymmetry, bond stretching/compressing/bending, rotation about a molecular bond--all these things can and do absord energy from a collision), and they negate the effects of all intermolecular forces, like dipole interations, hydrogen bonding, London dispersion forces, etc.\n\nIn gases like helium, the atoms are basically spherically symmetric, and most of these random forces are neglible.  Hence, ideal gas laws work really well for these--only at really ridiculously low temperatures and high pressures do these forces manage to liquify helium.  The larger you molecule is--and I'm not talking about mass so much as the number of chemical bonds--the less ideally it behaves.  The greater the heterogeneity of a gass, the less ideally it behaves.  The greater the polarity (eg seperation of charges) displayed by the molecule, the less ideally it behaves.
94789
Use Boyle's Law for that. Assuming the temperature is always constant, the product of pressure and volume is always constant.\n\nP * V = k\nor\nP1 * V1 = P2 * V2\n\nIf temperature is included in the equation, you could either use the combined gas law or the ideal gas law.\n\nNote: Elevation plays a significant role in Boyle's Law so it will have a difference in the gauge readings if you relocate it from sea level to the mountaintop.
542119
As described by the ideal gass laws, P1 V1 = P2 V2. This means that, as the pressure increases, the voulume of the contained vapor decreases and condences.
889941
Use the state equation of the ideal gases and solve for volume V:\n\np*V = n*R*T, V = n*R*T/p\n\nNow p = 657 Torr = 657/760 atm = 0.86 atm and R = 0.082 L*atm/mol*K, T = 283.8 oC = (283.8 + 273) K = 556.8 K so:\n\nV = 2.82*0.082*556.8/0.86 = 148.940 L
24946
For gases, we speak of "standard gas density." This is the density of the gas (expressed in grams per liter) at STP. If you discuss gas density at any other set of conditions, you drop the word standard and specify the pressure and temperature. Also, when you say "standard gas density," you do not need to add "at STP." STP is part of the definition of the term. It does no harm to say "standard gas density at STP," it just looks a bit silly. \n\nYou can calculate the ideal standard gas density fairly easily. Just take the mass of one mole of the gas and divide by the molar volume. \n\nMore explanation at the site linked below.
765323
I am not sure what you mean by "General Gas Laws."  The only law dealt with in physics is the Ideal Gas Law which says that pressure and volume are related to amount of gas, temperature and some constant.\n\nPV = nRT
147206
were do you start from? ideal quantum gas?\n\nwhat i know is: if you have managed to compute entropy S, heat capacity c is simply:\n\nc = T ∂S/∂T
712158
questioner didnt say the gas becomes ideal when volume is increased. he said it MORE CLOSELY approximates.\n\nthis is due to a pressure decrease at constant temperature. (boyle's law). less pressure, atoms further apart, less intermolecular attractions.\n\ncomplete absence of intermolecular forces is a required term in ideal gas principle. so reducing the force obviously creates a more ideal gas.
1185549
The first law of thermodynamics says that the total quantity of energy in the universe remains constant. This is the principle of the conservation of energy. The second law of thermodynamics states that the quality of this energy is degraded irreversibly. This is the principle of the degradation of energy.
827958
The first part is correct.  If the numbers in the second part are correct, it is true only for an ideal gas.  Other materials have various densities in their liquid and solid states.
695888
I assume the temperature is high enough that the O2 & Ne behave as ideal gases.\n\nThe partial pressure of each gas in a mixture of gases is proportional to its mole fraction.\n\nMoles of Ne = 12.6/20.18 = 0.6244\nMoles of O2 = 7.10/32.00 = 0.2219\nTotal moles = 0.6244 + 0.2219 = 0.8463\nMole fraction of Ne = 0.6244/0.8463 = 0.7378\nPartial pressure of Ne = 0.7378*0.435 = 0.321 atm (answer)\nMole fraction of O2 = 0.2219/0.8463 = 0.2622\nPartial pressure of O2 = 0.2622*0.435 = 0.114 atm\nTo check to make sure there are no errors:  0.114 + 0.321 = 0.435